ANSWER
The final volume of the balloon is 12.67L
EXPLANATION
Given that;
The initial volume of the ballon is 12dm^3
The initial temperature at STP is 273.15 degrees Celcius
The initial pressure at STP is 760 mmHg
The final temperature is 0 degrees Celcius
The final volume is 720 mmHg
Follow the steps below to find the new volume of the balloon
Step1; Write the general gas law equation
[tex]\text{ }\frac{\text{ P1 V1}}{\text{ T1}}=\text{ }\frac{\text{ P2V2}}{\text{ T2}}[/tex]Step 2; Convert the volume and temperature to liters and degrees Kelvin
[tex]\begin{gathered} \text{ 1dm}^3\text{ }=\text{ 1L} \\ \text{ Hence, 12dm}^3\text{ is equivalent to 12L} \\ \\ \text{ The final temperature is 0}\degree C \\ \text{ T = t + 273.15} \\ \text{ T = 0 + 273.15} \\ \text{ T = 273.15K} \end{gathered}[/tex]Step 3; Substitute the given data into the formula above to find the final volume
[tex]\begin{gathered} \text{ }\frac{\text{ P1V1}}{\text{ T1}}\text{ }=\text{ }\frac{\text{ P2 V2}}{\text{ T2}} \\ \\ \text{ }\frac{760\times\text{ 12}}{273.15}\text{ }=\frac{720\times V2}{273.15} \\ \text{ Cross multiply} \\ \text{ 760 }\times\text{ 12 }\times\text{ 273.15 }=\text{ 720 }\times\text{ V2 }\times\text{ 273.15} \\ \text{ Isolate V2} \\ \text{ V2 }=\text{ }\frac{760\text{ }\times\text{ 12}\times\text{ 273.15}}{720\text{ }\times\text{ 273.15}} \\ \text{ } \\ \text{ V2}=\frac{760\times12\times\cancel{273.15}}{720\times\cancel{273.15}} \\ \text{ } \\ \text{ V2 }=\text{ }\frac{9120}{720} \\ \text{ V2 = 12.67L} \end{gathered}[/tex]Hence, the final volume of the balloon is 12.67L
how do i order elements from smallest to largest atomic radius..Sc, Co, Ca, Br, K
Please, look at the next picture:
The image above shows us how the atomic size increases.
According to this, the order from the smallest to the largest is:
Br
Co
Sc
Ca
K
Answer:
Br
Co
Sc
Ca
K
A chemist used 65.5 mL of a sodium phosphate stock solution to make up 0.675 M sodium phosphate in a 450 mL volumetric flask. What is the molarity of the original stock solution?
ANSWER
The concentration of the original stock solution is 0.09825M
EXPLANATION
Given that;
The initial volume of the stock solution is 450mL
The molarity of the solution prepared is 0.675M
The volume of the solution used is 65.5mL
Follow the steps below to find the molarity of the original stock solution.
Step 1; Use the dilution formula
[tex]\text{ M1 V1 }=\text{ M2V2}[/tex]Where
M1 is the initial molarity of the solution
V1 is the initial volume of the solution
M2 is the final concentration of the solution
V2 is the final volume of the solution.
Step 2; Convert the volume to liters from mL
Recall, that 1 mL is 0.001L
Hence,
V1 = 450 x 0.001
V1 = 0.45L
V2 = 65.5 x 0.001
V2 = 0.0655L
Step 3; Substitute the given data into the dilution formula in step 1
[tex]\begin{gathered} \text{ M1 V1 }=\text{ M2V2} \\ 0.45\text{ }\times\text{ M1}=\text{ 0.675}\times0.0655 \\ \text{ 0.45M1 }=\text{ 0.0442} \\ \text{ Divide both sides by 0.45} \\ \frac{\cancel{0.45}\times M1}{\cancel{0.45}}=\text{ }\frac{0.0442}{0.45} \\ \text{ M1 }=0.09825\text{ M} \end{gathered}[/tex]Therefore, the concentration of the original stock solution is 0.09825M
3. How much Heat must be added to a 10 gram sample of Gold to increase itstemperature by 5 C. The Specific Heat of Gold is 0.13 J/g C
6.5Joules
Explanations:The formula for calculating the amount of heat that must be added is expressed as:
[tex]Q=mc\triangle t[/tex]where:
• m is the ,mass ,of the object
,• c is the s,pecific heat capacity
,• △t is the ,change in temperature
Given the following parameters
m = 10grams
c = 0.13 J/g C
△t = 5 C
Substitute the given parameters into the formula
[tex]\begin{gathered} Q=10\cancel{g}\times\frac{0.13J}{\cancel{g}^\cancel{^0C}}\times5\cancel{^0C}^ \\ Q=10\times0.13J\times5 \\ Q=1.3\times5 \\ Q=6.5Joules \end{gathered}[/tex]This shows that 6.5Joules of heat must be added to a 10 gram sample of Gold to increase its temperature by 5 C.
An automobile engine generates 2156 Joules of heat that must be carried away by the cooling system. The internal energy changes by -2722 Joules in thisCalculate w for the engine. This represents the work available to push the pistons in this process.Work =____j
Explanation:
According to the first law of thermodynamics.
ΔE = q + W
Where ΔE is the change in internal energy, q is the heat absorbed or released by the system and W is the work done on or by the system.
We know that the automobile engine is generating 2156 J and those Joules are being carried away by the cooling system. Since that heat is going out of the system it must be negative.
q = - 2156 J
The internal energy changes -2722 J.
ΔE = -2722 J
Finally we can replace these values in the formula and solve it for the work to get the answer to our problem.
ΔE = q + W
W = ΔE - q
W = -2722 J - (-2156 J)
W = -566 J
Answer: Work = - 566 J
What Celsius temperature, T2 , is required to change the volume of the gas sample in Part A ( T1 = 35 ∘C , V1 = 1260 L ) to a volume of 2520 L ? Assume no change in pressure or the amount of gas in the balloon.
70 degree celsius
Explanations:According to Charle's law, the volume of a given mass of gas is directly proportional to absolute temperature provided that the pressure is constant. Mathematically;
[tex]\begin{gathered} v\alpha T \\ v=kT \\ k=\frac{v_1}{T_1}=\frac{v_2}{T_2} \end{gathered}[/tex]where
v1 and v2 are the initial and final volume respectively
T1 and T2 are the initial and final temperature respectively
Given the following parameters
[tex]\begin{gathered} v_1=1260L \\ v_2=2520L \\ T_1=35^0C \end{gathered}[/tex]Required
Final temperature T2
Substitute the given parameters into the formula to have:
[tex]\begin{gathered} T_2=\frac{v_2T_1}{v_1} \\ T_2=\frac{2520\times35}{1260} \\ T_2=70^0C \end{gathered}[/tex]Hence the celsius temperature T2 required is 70 degree celsius
22.What number should be placed in front of the H2O in the reaction below?2 Fe(OH)3 ---> Fe2O3 + ___ H2OSelect one:a. 1b. 2c. 3d. 6
Answer
C. 3
Explanation
On the left side there are 6 oxygens and 6 hydrogens. Then on the right side there should be the same number of atoms, if we add 3 infront of H2O, there will be 6 oxygens and 6 hydrogens.
A 245.9 mL balloon has a pressure of 0.867 atm. If the pressure changes to 1.459 atm, what is the new volume in mL of the balloon? Final answers must have correct significant figures and units to receive full credit. Partial credit may be awarded if appropriate work is shown.
In this question, we have an example of Boyle's gas law, which is an experimental gas law that shows the relationship between pressure and volume of gases, the formula is:
P1V1 = P2V2
We have:
P1 = 0.867 atm
V1 = 245.9 mL
P2 = 1.459 atm
V2 = ?
Now we add these values into the formula:
0.867 * 245.9 = 1.459 * V2
V2 = 146 mL
What is the skeletal equation? I have the word equation just need the skeletal for question number e
In word equation, you need to write the name of each compound, reactants and products. In this case, it is:
Word:
Aluminum + Copper (II) Chloride --> Copper + Aluminum
chloride
The skeleton equation you must put the formulas of the compounds written in word equation.
Skeleton:
Al(s) + CuCl2(aq) --> Cu(s) + AlCl3(aq)
Answer:
Word:
Aluminum + Copper (II) Chloride --> Copper + Aluminum
chloride
Skeleton:
Al(s) + CuCl2(aq) --> Cu(s) + AlCl3(aq)
1) ____Al + ____ Cl₂ _____ AlCl₃If 25.0 moles of chlorine is used, how many grams of aluminum chloride can be produced?
Step 1
The reaction must be written and balanced:
2Al + 3Cl2 2 AlCl3
-----------------
Step 2
Information provided: 25.0 moles Cl2
Information needed: the molar mass of AlCl3 => 133 g/mol
-----------------
Step 3
By stoichiometry
1 mole AlCl3 = 133 g/mol
Procedure:
3 x 1 mole Cl2 --------- 2 x 133 g AlCl3
25.0 moles Cl2 --------- X
X = 25.0 moles Cl2 x 2 x 133 g AlCl3/3 x 1 mole Cl2 = 2217 g AlCl3
Answer: 2217 g AlCl3
how to calculate the percentage yield
The yield percentage corresponds to the actual quantity of products obtained over the theoretical amount of product that should be produced. It can be expressed with the following formula.
[tex]\text{Yield percentage}=\frac{\text{Actual yield}}{Theoretical\text{ yield}}\times100\%[/tex]Now, the actual yield obtained is found experimentally, generally, it is a datum given to you.
The theoretical yield to be obtained will depend on the stoichiometry of the reaction. If we have for example the following reaction:
[tex]aA+bB\rightarrow cC+dD[/tex]If they give us the moles of reactant A and ask us to find the moles of C that will be formed, we must see the ratio C to A, which in this case will be c/a and the moles of C formed will be:
[tex]\text{Moles C}=givenMolA\times\frac{cMolC}{aMolA}=\text{Theoretical yield}[/tex]By having the two values, the actual yield and the theoretical yield, we can find the percentage yield with the first equation.
Topic 5-A generic example of an equilibrium reaction is shown below.Answer the following questions about what direction equilibrium shiftaccording to Le Chatelier's principle.A+B=C+D+heata. Removing some of compound AAb. Increasing the temperaturec. Adding more of compound DDd. Increasing concentration of compound BBe. Decreasing the temperature
a) Towards the left
b) Towards the left
c) Towards the left
d) Towards the right
e) Towards the right
Explanations:What is the Le Chatelier's principle?This prnciple states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium.
According to the equation shown below;
[tex]A+B\rightarrow C+D+heat[/tex]a) Removing some of the compound A means the total concentration of the reactant will reduce and be less than the product. In order to establish equilibrium, the equilibrium position will shift to the side with less amount of concentration of compound (in this case, the reactant side which is towards the left)
b) Increasing the temperature will decrease the equlibrium constant. This will favor the endothermic reaction (heat absorbed from the surroundings) and as such the equilibrium will shift to the left to absorb the added energy to the reactant.
c) Adding more compound D to the product will favour the backward reaction since the total concentration of the product will increase and be more than the reactant. In order to establish equilibrium, the equilibrium position will shift to the side with less amount of concentration of compound (in this case, the reactant side which is towards the left).
d) Increasing concentration of compound B (the reactant) will favor the forward reaction and as such the equilibrium position shifting to the right in order to establish equilibrium.
e) Decreasing the temperature will increase the equlibrium constant. This will favor the exothermic reaction (heat released to the surroundings) and the equilibrium will shift to the right
Which of the changes listed below would shift the following reaction to the right?4HCl(g) + O2(g) ➡️⬅️ 2Cl2(g) + 2H2O(g)Decrease of pressure Removal of O2Addition of Cl2Increase of pressure
Answer
Increase of pressure
Explanation
In accordance with Le Châtelier’s principle, a shift in the equilibrium that reduces the total number of molecules per unit of volume will be favored because this relieves the stress. The reverse reaction would be favored by a decrease in pressure.
I need help with the picture, the top part is cut out but it wasn’t important
Asuming the groung state is A the energy of the electron in the ground state is 450zJ, Then the first nergy leve is B where the energy of the electron is 900zJ. If an electron jumps from a lower level to a higher level (like in the picture) it needs to absorb energy.
For both substances A and B, which states of matter are shown on the graph? A) gas and liquid onlyB)liquid and solid onlyC) gas, fusion, liquid, vaporization, and solidD) gas, liquid and solid
From the given graph, it can be seen the representation of the process of going from one state of matter to other one.
For both A and B, they start at a solid state.
Then, they go through a fusion process and became liquids.
After that, they suffer vaporization and turn into gases.
From this, we can conclude that the states of matter shown are gas, liquid and solid.
The correct answer is D) gas, liquid and solid.
Question 1 of 10How many moles of ammonia would be required to react exactly with0.876 moles of copper(ll) oxide in the following chemical reaction?2 NH (g) + 3 CuO(s) – 3 Cu(s) + N,(g) + 3 H Og)
Given the balanced equation:
• 2 NH₃(g) + 3 CuO(s) → 3 Cu(s) + N₂(g) + 3 H₂O(g)
0. The coefficients tell you the mole ratios, so 2 moles ammonia (NH3) will react with 3 moles of copper(II) oxide, (CuO).
,1. We will set up a simple proportion in order to solve this , as follows:
• 2 mol NH3/3 mol CuO = x mol NH3/0.876mol CuO.
→0.876molCuO * 2molNH3/3molCuO=0.584 molesNH3
• This means that 0.584 moles of Ammonia, would be required to react exactly with 0.876 moles of copper(II) oxide.
Li3N(s) + 3H2O(l) → NH3(g) + 3LiOH(aq) What mass of water is needed to react with 98.7 grams of lithium nitride?
Step 1
The reaction must be written, completed, and balanced:
Li3N(s) + 3H2O(l) → NH3(g) + 3LiOH(aq)
----------
Step 2
Information provided:
The mass of Li3N = 98.7 g
Information needed:
The molar masses,
Li3N) 34.8 g/mol
H2O) 18.0 g/mol
----------
Step 3
By stoichiometry,
1 mole Li3N = 34.8 g
1 mole H2O = 18.0 g
Procedure:
Li3N(s) + 3H2O(l) → NH3(g) + 3LiOH(aq)
34.8 g Li3N ---------- 3 x 18.0 g H2O
98.7 g Li3N ----------- X
X = 98.7 g Li3N x 3 x 18.0 g H2O/34.8 g Li3N = 153 g approx.
Answer: 153 g of water
in the reaction 2CO(g) + O (g) → 2CO (g), how many moles of CO2 can be produced from 5.0 moles of CO and 6.0 moles of O2?
For this stoichiometry problem, we need to first, set up the properly balanced equation, which the question already provided us:
2 CO + O2 -> 2 CO2
We have:
5.0 moles of CO
6.0 moles of O2
Notice that we have two values for the reactants, this means that we need to find which one is the limiting and which one will be the excess reactant, let's try CO first:
From the molar ratio of the reaction, which is 2:1, 2 moles of CO for 1 mol of O2, we need to see if it makes sense 5 moles of CO for 6 moles of O2
2 CO = 1 O2
5 CO = x O2
x = 2.5 moles, therefore we have O2 in excess, since we only need 2.5 moles of O2 to react with 5 moles of CO
Using the limiting reactant, 5 moles of CO, now we can identify the number of moles of CO2, by the molar ratio between CO and CO2, which is 2:2, 2 moles of CO will produce 5 moles of CO2, therefore if we have 5 moles of CO, we will also have 5 moles of CO2
It will be produced 5 moles of CO2
A student is making a solution of sugar in water. If the student uses 0.49 moles of sugar and enough water to make 442.80 milliliters of solution, what is the molarity of the student's sugar solution? Round your answer to the nearest 0.01 and include units properly abbreviated, but NOT substance!
Step 1
Molarity is defined as:
Molarity (M or mol/L) = moles of solute (sugar)/volume of the solution (L)
---------
Step 2
Information provided:
Moles of sugar = 0.49 moles
Volume of the solution = 442.80 mL x (1 L/1000 mL) = 0.44280 L
(1 L = 1000 mL)
---------
Step 3
Procedure:
Molarity = 0.49 moles/0.44280 L = 1.10 mol/L
Answer: Molarity = 1.10 mol/L
Covalent Bonding is characterized by...Group of answer choicesLarge crystalsElectron sharingMetals with non-metalsElectron transfer
1) Covalent bonds.
Atoms bond to other atoms to make molecules. They can do it in several ways, one of them being covalent bonds. In this type of bond, the atoms involved share electrons.
When 0.201 g of sodium metal is added to an excess of hydrochloride acid, 2090 J of heat are produced. What is the enthalpy of the reaction as written? 2Na(s) + 2HCI(aq) + H2(g)Enthalpy of reaction = ___________ kJ
-239.13kJ/mol
Explanations:The complete chemical reaction between the sodium metal and hydrochloric acid is expressed as shown:
[tex]2Na(s)+2\text{HCl(aq)}\rightarrow2NaCl(aq)+H_2(g)[/tex]The enthalpy of the reaction is expressed using the formula;
[tex]\triangle H^0_{rxn}=\frac{Quantity\text{ of h}eat}{Moles\text{ of sodium}}[/tex]Given that quantity of energy released is -2090J (Since energy is released by the system)
Get the moles of sodium
[tex]\begin{gathered} Moles\text{ of sodium =}\frac{Mass\text{ of Na}}{Molar\text{ mass of Na}} \\ \text{Moles of sodium =}\frac{0.201g}{22.99\text{g/mol}} \\ \text{Moles of sodium = }0.00874\text{moles of Na} \end{gathered}[/tex]Next is to get the required enthalpy of the reaction in kJ/mol
[tex]\begin{gathered} \text{Enthalpy of the reaction = }\frac{-2.090kJ}{0.00874\text{mol}} \\ \text{Enthalpy of the reaction = -}239.13\text{kJ/mol} \end{gathered}[/tex]Hence the enthalpy of the reaction is -239.13kJ/mol
A 38.3 L sample of gas at 30.4*C and 273.5 mm ahh expands to 256.9 L at 18.2*C. What is the new gas pressure?A. 39.1 B.24.4 C.42.5 D.2.44
Explanation:
We have a sample of gas that at 30.4 °C and 273.5 mmHg of pressure occupies 38.3 L. The gas expands to 256.9 L at 18.2 °C.
We are working with a gas and we know the initial conditions of temperature, pressure and volume, and know the final temperature and volume but not the pressure. We can apply the following formula.
P₁ * V₁/T₁ = P₂ * V₂/T₂
Where P₁, V₁ and T₁ are the initial conditions and P₂, V₂ and T₂ are the final conditions. We know the values of them, and we can convert the temperature from °C to K.
P₁ = 273.5 mmHg
V₁ = 38.3 L
T₁ = (30.4 + 273.15) K
T₁ = 303.55 K
P₂= ?
V₂ = 256.9 L
T₂ = (18.2 + 273.15)
T₂ = 291.35 K
We can replace these values in the formula and solve it for the final volume.
P₁ * V₁/T₁ = P₂ * V₂/T₂
P₂ = (P₁ * V₁ * T₂)/(T₁ * V₂)
P₂ = (273.5 mmHg * 38.3 L * 303.55 K)/(291.35 K * 256.9 L)
P₂ = 42.5 mmHg
Answer: c. 42.5 mmHg
Can somebody help me solve this ? I dont get how to do it
Answer:
The mass of water is 25.9g.
Explanation:
1st) It is necessary to use the Heat formula. Knowing that the piece of aluminum releases heat and the water absorbs heat, the equation is a sum of both heats euqal to zero:
[tex]Q_{Al}+Q_{water}=0[/tex]2nd) The information given in the exercise is:
• Piece of aluminum:
- Mass (mAl)=55.0g
- Heat capacity (cAl)=0.902J/°C*g
- Initial Temperature (TiAl)= 72.4°C
- Final Temperature (TfAl)= 44.9°C
• Water:
- Mass (mwater)= this is what we have to calculate.
- Heat capacity (cwater)= 4.18J/°C*g
- Initial Temperature (Tiwater)= 32.3°C
- Final Temperature (Tfwater)= 44.9°C
3rd) It is necessary to replace the values in the formula to calculate the mass of the aluminum piece:
[tex]\begin{gathered} -Q_{Al}=Q_{water} \\ -\lbrack m_{Al}*c_{Al}*(T_{fAl}-T_{iAl})\rbrack=m_{water}*c_{water}*\left(T_{fwater}-T_{iwater}\right) \\ -\lbrack55.0g*0.902\frac{J}{\degree C*g}*(44.9°C-72.4°C)\rbrack=m_{water}*4.18\frac{J}{\operatorname{\degree}C*g}*(44.9°C-32.3°C) \\ -\lbrack-1364.28J\rbrack=m_{water}*52.67\frac{J}{\operatorname{\degree}C} \\ \frac{1364.28J}{52.67\frac{J}{g}}=m_{water} \\ m_{water}=25.9g \\ \end{gathered}[/tex]Resolution number 2 (image):
Finally, the mass of water is 25.9g.
2) A gas is held in a sealed glass container. The initial pressure and temperature are 0.150 atm and 72 ° C. If the final temperature is 157 ° C, what is the final pressure (in atmospheres)?
Answer:
The final pressure is 0.3297atm.
Explanation:
1st) The given information from the exercise is:
- Initial pressure (P1): 0.150atm
- Initial temperature (T1): 72°C
- Final temperature (T2): 157°C
2nd) To calculate the final pressure, we can use the Gay-Lussac's formula, by replacing the values:
[tex]\begin{gathered} \frac{P_1}{T_1}=\frac{P_2}{T_2} \\ \frac{0.150atm}{72°C}=\frac{P_2}{157°C} \\ 0.0021\frac{atm}{°C}=\frac{P_2}{157°C} \\ 0.0021\frac{atm}{°C}*157°C=P_2 \\ 0.3297atm=P_2 \end{gathered}[/tex]So, the final pressure is 0.3297atm.
26.Which of the following pH values represents the largest number of H+ ions?Select one:a. 1b. 5c. 9d. 13
ANSWER
Option
EXPLANATION
pH measures the acidity and alkalinity of a substance
The pH of the acid decreases from 1 to 7 on the pH scale while the pH of the base increases from 7 to 14 to increases
Recall, that a strong acid has pH value ranging from 1 to 3
Strong acid is defined as the type of acid which will produce hydrogen ions as the only positive ions when completely dissolved in water. This implies that strong acid has the largest number of hydrogen ions (H+). Therefore, a substance with pH value 1 will have the largest number of hydrogen ions
Hence, the correct answer is option A
(The question is in the photo Sorry lol) A 21 L tank contains a gas under a pressure of 367 atm. What volume would the gas occupy at the same temperature at 630 torr of pressure?Answer in units of L.✨Please leave all the numbers after the decimal in the final answer
Again, this is Boyles Law, since we want V2 from given:
V1 = 21 L
P1 = 367 atm
P2 = 630 torr = 0.828947 atm
V2 = ?
Remember to covert torr to atm so that the units are the same and can cancel one another.
1 torr = 0,00131579 atm
630 torr = 0.828947 atm
And the temperature is constant, so we do not need to use it.
P1V1 = P2V2
V2 = P1V1/P2
V2 = (367 atm x 21 L)/0.828947 atm
V2 = 9297.337465 L
Polarity and solubility.is water polar, nonpolar, or ionic?is Vinegar polar, nonpolar, or ionic?is iodine solution polar, nonpolar, or ionic?is rubbing alcohol polar, nonpolar, or ionic?is vegetable oil polar, nonpolar, or ionic?
In order to determine if a compound is polar, nonpolar, or ionic, we need to look at the main component of this compound and see the difference in the electronegativity between the elements, if the difference (which can be easily found in many tables online) between the electronegativity if high, then we have an ionic compound, if it is very low, then we have a nonpolar compound, if it falls in the middle, we have a polar compound.
For water, we have H and O, which are not high to be an ionic compound and not low enough to be nonpolar, as water is known the best polar solvent, water is a polar compound
Acetic acid is the main component of vinegar, and since it is an acid, it is also a polar substance and has a high solubility in water
Iodine solution is classified as nonpolar due to its concentration of elemental iodine, and it is better dissolved in oil
Alcohol substances are made with the same type of components as water, O and H, which also makes it polar
Vegetable oil, as an oil it is nonpolar, most oils are nonpolar
Therefore we have:
Water - polar
Vinegar - polar
Iodine - nonpolar
Alcohol - polar
Vegetable oil - nonpolar
How many liters are in 2.78x10^-3 moles of oxygen gas
ANSWER
The volume of oxygen gas is 0.062272L
STEP-BY-STEP EXPLANATION:
Given information
[tex]\text{The number of moles of oxygen gas = 2.78 }\times10^{-3}\text{ moles}[/tex]Recall that, at ST, 1 mole is equivalent to 22.4L
Let x represents the volume of oxygen
[tex]\begin{gathered} 1\text{ mole }\rightarrow\text{ 22.4L} \\ 2.78\text{ }\times10^{-3}\text{ }\rightarrow\text{ xL} \\ \text{cross multiply} \\ 1\text{ }\times\text{ x = 22.4 }\times\text{ 2.78 }\times10^{-3} \\ x\text{ = 62.272 }\times10^{-3} \\ x\text{ = 6.2272 }\times10^{-2}L \end{gathered}[/tex][tex]\text{Therefore, the volume of oxygen gas is 6.2272 }\times10^{-2}L[/tex]AN
. Given the following reaction: ___N2 (g) + ___H2 (g)→___ NH3 (g)If 2.00 L of ammonia (NH3) are produced in the reaction between nitrogen and hydrogen at STP, how many liters of nitrogen gas is used up in this reaction?
In this question, we have to find how many liters of Nitrogen gas is used to make 2.00 Liters of NH3, and the first thing we have to do is set up the properly balanced equation:
N2 + 3 H2 -> 2 NH3, now the reaction is balanced
According to the balanced equation, the molar ratio between NH3 and N2 is 2:1, which means with 1 mol of N2, we can produce 2 moles of NH3, but now we have to match the number of moles equivalent to 2 Liters of NH3
At STP (Standard Temperature and Pressure), 1 mol of gas is equal to 22.4 Liters of Volume, which means, 2 moles of gas will be equal to:
22.4 L = 1 mol
2 L = x moles
x = 0.089 moles of NH3 in 2 Liters
Now, according to the molar ratio, if we have 0.089 moles of NH3, we will have:
2 NH3 = 1 N2
0.089 NH3 = x N2
x = 0.0445 moles of N2
Now to find the volume, we will use that information about STP again
1 mol = 22.4 Liters
0.0445 moles = x Liters
x = 1 Liter of Nitrogen gas is required
How are the temperature, pressure, amount and volume of gas related to each other in the gas laws?Hypotheses:
Talking about ideal gases, we can espress the following relations:
This table tells us that:
1. When temperature is constant, pressure and volume are inversely proportional. This means that when pressure decreases, volume increases and when pressure increases, volume decreases.
2. When pressure is constant, volume and temperature are directly proportional. This means that if volume increases, temperature increases and if volume decreases, temperature also does.
3. When volume is constant, pressure and temperature are directly proportional. This means that if pressure increases, temperature increases and if presure decreases, temperature also does.
A 410 L volume of nitrogen gas is cooled from 61 C to -25 C. What is the volume of the nitrogen at the lower temperature if all volumes are measured at the same pressure?
Answer:
[tex]304.5\text{L}[/tex]Explanation:
Here, we want to get the volume of the nitrogen gas at the lower temperature
From Charles' law, we know that volume and temperature (in Kelvin) are directly proportion
The mathematical relationship is:
[tex]\frac{V_1}{T_1}\text{ = }\frac{V_2}{T_2}[/tex]Where:
V1 is the initial volume which is 410 L
V2 is the final volume which is unknown
T1 is the initial temperature which we will convert to Kelvin by adding 273.15 K, we have it as 61 + 273.15 = 334.15 K
T2 is the final temperature which we have to convert to Kelvin by adding it to 273.15K : We have that as -25 + 273.15 = 248.15 K
Substituting the values, we have it that:
[tex]\begin{gathered} \frac{410}{334.15}\text{ = }\frac{V_2}{248.15} \\ \\ V_2\text{ = }\frac{248.15\text{ }\times410}{334.15} \\ \\ V_2\text{ = 304.5 L} \end{gathered}[/tex]