Answer:
A
Explanation:
Reactants are on the right side of the chemical reaction
How many moles of aluminum oxide (Al2O3) will be produced if 1.5 mole of aluminum (AI) reacts with oxygen? Input a numerical answer only. 4Al + 302 ---> 2Al2O3
Explanation:
The number of moles of Al2O3 formed is approximately 4.25 moles. Second find the limiting reactant. Since O2 has less value that is 2.126 than Al that is 2.287, O2 is the limiting reactant in this reaction.
Can someone help me out, thanks
Answer:
See EXPLANATION
Explanation:
We must bear in mind that in balancing chemical reaction equations, the number of atoms of each element on the right hand side must be the same as the number of atoms of the same element on the left hand side of the reaction equation. This follows from the law of conservation of mass.
Based on this;
There are two oxygen atoms on the left hand side of the reaction equation, thus total mass of oxygen = 2 * 16 amu = 32 amu
There are two oxygen atoms on the product side of the reaction equation, thus the total mass of oxygen = 2 * 16 amu = 32 amu
i cant seem to figure out ANY of these... help when you can pls :.)
Oxygen and ozone are allowed to come to equilibrium in the exothermic reaction 2O3(g) <--> 3O2(g) Which change will increase the numerical value of the equilibrium constant, K
Answer:
don't get the question2
.......state Hess law
Why is the regression equation not exactly y = 100 • 0.5n?
Answer:
Radioactive decay is a random event.
Explanation:
on edge
Answer:
Radioactive decay is a random event.
Explanation:
Edge 2020
PLEASE HELP I HAVE 19 MINUTES LEFT I WILL MARK BRAINLIEST
How much more acidic is a pH of 4 as compared to a pH of 6.5?
Answer:
316.227766
Explanation:
What is the partial pressure (in atm) of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 60.0 grams CO₂, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?
Answer:
2.09 atm
Explanation:
Step 1: Given and required data
Mass of CO₂ (m): 60.0 gVolume of the vessel (V): 25.0 LTemperature (T): 468.2 KWe won't need the data of water and uncombusted fuel, since the partial pressures are independent of each other.
Step 2: Calculate the number of moles (n) corresponding to 60.0 g of CO₂
The molar mass of CO₂ is 44.01 g/mol.
60.0 g × 1 mol/44.01 g = 1.36 mol
Step 3: Calculate the partial pressure of CO₂
We will use the ideal gas equation.
P × V = n × R × T
P = n × R × T/ V
P = 1.36 mol × (0.0821 atm.L/mol.K) × 468.2 K/ 25.0 L = 2.09 atm
The partial pressure of [tex]\rm CO_2[/tex] in 25 L fuel combustion vessel has been 2.09 atm.
From the ideal gas equation:
PV =nRT
P= partial pressure
V = volume = 25 L
n = moles of carbon dioxide
Moles = [tex]\rm \dfrac{weight}{molecular\;weight}[/tex]
Moles of [tex]\rm CO_2[/tex] = [tex]\rm \dfrac{60}{44}[/tex] mol
Moles of [tex]\rm CO_2[/tex] = 1.36 mol
R = constant = 0.0821 atm.L/mol.K
T = temperature in Kelvin = 468.2 K
Partial pressure of [tex]\rm CO_2[/tex] = [tex]\rm \dfrac{1.36\;\times\0.0821\;\times\;468.2}{25}[/tex]
Partial pressure of [tex]\rm CO_2[/tex] = 2.09 atm.
The partial pressure of [tex]\rm CO_2[/tex] in 25 L fuel combustion vessel has been 2.09 atm.
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when rolling a number cube 500 times, how many times you expect to get a 3?
Answer:
[tex]\frac{250}{3}[/tex]
Explanation:
you can expect to get a 3 (theoretically) 1 time every 6 times you roll. A 1/6 chance.
Here's the equation:
[tex]\frac{1}{6} =\frac{x}{500}[/tex]
cross multiply (i think that's what it is called)
500=6x
divide by 6 on both sides:
x=[tex]\frac{250}{3}[/tex] or approx 83 times.
Hope this helps! Lmk if u have more questions <3
1. In a chemical reaction
a. the mass of the reactants equals the mass of the products.
b. the mass of the products is greater than the mass of reactants.
c.the number of atoms in the reactants and products must change.
d. energy as heat must be added to the reactants.
Answer:
A
Explanation:
Law of conservation of matter
A common asteroid is in the first photograph. Haley's Comet is in the second photograph. What can be inferred about comets and asteroids? Answer A Both have orbits around the Earth that are ellipses B Both are miniature planets because they orbit the Sun C Both could be planetary fragments from the beginnings of solar system formation D Both are made of rock, ice, and solar dust from the beginning of the solar system
Answer:
D Both are made of rock ,ice and solar dust from the beginning of the solar system
Answer:
The answer is D
Explanation:
Calculate the [H+] in a solution that has a pH or 5.21
Answer:
[H⁺] = 6.17×10¯⁶ M
Explanation:
From the question given above, the following data were obtained:
pH = 5.21
Concentration of Hydrogen ion [H⁺] =?
The pH of a solution is defined by the following equation:
pH = –Log [H⁺]
With the above formula, we can obtain the concentration of Hydrogen ion [H⁺] in the solution as follow:
pH = –Log [H⁺]
5.21 = –Log [H⁺]
Divide both side by –1
–5.21 = Log [H⁺]
Take the antilog of –5.21
[H⁺] = Antilog (–5.21)
[H⁺] = 6.17×10¯⁶ M
Therefore, the concentration of Hydrogen ion [H⁺] in the solution is 6.17×10¯⁶ M
Inquiry Extension Consider a reaction that occurs between solid potassium and chlorine gas. If you start with an initial mass of 15.20 g K, and an initial mass of 2.830 g Cl2, calculate which reactant is limiting. Explain how to determine how much more of the limiting reactant would be needed to completely consume the excess reactant. Verify your explanation with an example
The 3.13 g of K would be needed to completely react with the remaining [tex]Cl_2[/tex].
To determine which reactant is limiting, we need to calculate the amount of product that can be formed from each reactant and compare them. The reactant that produces less product is the limiting reactant, since the reaction cannot proceed further once it is consumed.
The balanced chemical equation for the reaction between solid potassium and chlorine gas is:
2 K(s) + [tex]Cl_2[/tex](g) -> 2 KCl(s)
From the equation, we can see that 2 moles of K react with 1 mole of [tex]Cl_2[/tex] to form 2 moles of KCl.
First, we need to convert the masses of K and [tex]Cl_2[/tex] into moles:
moles of K = 15.20 g / 39.10 g/mol = 0.388 mol
moles of [tex]Cl_2[/tex] = 2.830 g / 70.90 g/mol = 0.040 mol
Now, we can use the mole ratio from the balanced equation to calculate the theoretical yield of KCl from each reactant:
Theoretical yield of KCl from K: 0.388 mol K x (2 mol KCl / 2 mol K) = 0.388 mol KCl
Theoretical yield of KCl from [tex]Cl_2[/tex]: 0.040 mol [tex]Cl_2[/tex] x (2 mol KCl / 1 mol [tex]Cl_2[/tex]) = 0.080 mol KCl
We can see that the theoretical yield of KCl from K is 0.388 mol, while the theoretical yield of KCl from [tex]Cl_2[/tex] is 0.080 mol. Therefore, the limiting reactant is [tex]Cl_2[/tex], since it produces less product.
To determine how much more of the limiting reactant would be needed to completely consume the excess reactant, we can use the stoichiometry of the balanced equation.
We know that 1 mole of [tex]Cl_2[/tex] reacts with 2 moles of K to produce 2 moles of KCl. Therefore, the amount of additional K needed to react with the remaining [tex]Cl_2[/tex] can be calculated as follows:
moles of K needed = 0.040 mol [tex]Cl_2[/tex] x (2 mol K / 1 mol [tex]Cl_2[/tex])
= 0.080 mol K
This means that 0.080 moles of K would be needed to completely consume the remaining [tex]Cl_2[/tex]. We can convert this to a mass by multiplying by the molar mass of K:
mass of K needed = 0.080 mol K x 39.10 g/mol
= 3.13 g K
Therefore, The 3.13 g of K would be needed to completely react with the remaining.
Example verification:
Suppose we had an additional 0.50 g of [tex]Cl_2[/tex] in the reaction. Would all of the K be consumed, or would there still be excess K?
Moles of additional [tex]Cl_2[/tex] = mass of [tex]Cl_2[/tex] / molar mass of [tex]Cl_2[/tex]
Moles of additional [tex]Cl_2[/tex] = 0.50 g / 70.90 g/mol
Moles of additional [tex]Cl_2[/tex] = 0.0070 mol
The theoretical yield of KCl that can be formed from the additional [tex]Cl_2[/tex] is:
0.0070 mol [tex]Cl_2[/tex] x (2 mol KCl / 1 mol [tex]Cl_2[/tex]) x (74.55 g KCl / 1 mol KCl) = 1.04 g KCl
Therefore, the total amount of KCl that can be formed from all of the [tex]Cl_2[/tex] is:
5.95 g + 1.04 g = 6.99 g
The amount of K that would be needed to completely consume all of the [tex]Cl_2[/tex].
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Calculate the volume of a gas sample at 273 K and 101.325 kPa if 455 cm of the gas are
collected at 36.0 °C and 97.0 kPa. What is the name of the gas law used in this calculation?
Answer:
The name of the game law used is called the Charles Law
Anyone knows gunpowder formula?
write half-reactions that show how H2O2 can act as either an oxidizing agent or a reducing agent, and describe where each of these situations occurred in your testing.
Answer:
H2O2 reduces itself to H2O and also oxidizes to O2 simultaneously thereby acting both as an oxidizing and reducing agent .
Explanation:
When
H2O2 acts as an oxidizing agent
H2O2 + 2e- 2H+---> 2H2O
Reducing agent
H2O2 --> O2 + 2e + 2H+
H2O2 reduces itself to H2O and also oxidizes to O2 simultaneously thereby acting both as an oxidizing and reducing agent .
Can someone please solve this question?? Is an element in group 3 likely to bond with an element from group 2?? Explain using the number of balance electrons from each element and the tot number of balance electrons needed to fill an about shell
Answer:
An atom with one or two valence electrons more than a closed shell The number of valence electrons of an element can be determined Groups 3-12 (transition metals), 2* (The 4s shell is complete and cannot hold any more electrons) in explaining the molecular structure of many organic compounds.
Explanation:
Guided Notes: Types of Chemical Reactions:
1. Synthesis or Combination
A + B à AB
Example:
Magnesium + Oxygen gas à Magnesium Oxide
_________ + _______ à __________
2. Decomposition
AB à A + B
Example:
Calcium Oxide à Calcium + Oxygen
_______ à __________ + __________
3. Single Replacement
A + BX à AX + B
Example:
_________ + _______ à __________ + __________
4. Double Replacement
AX + BY à AY + BX
Example:
_________ + _______ à __________ + _________
5. Combustion
CxHyOz + O2 à CO2 + H2O
Example:
Propane + Oxygen à Carbon dioxide + water
_________ + _______ à __________ + _________
Classify the following chemical reactions:
Sodium and Chlorine gas à Sodium Chloride
_________ + _______ à __________ Type of Reaction: __________________
CaCO3 + HCl à CaCl2 + H2CO3 Type of Reaction: __________________
Al + ZnCl2 à AlCl3 + Zn Type of Reaction: __________________
Fe + O2 à Fe2O3 Type of Reaction: __________________
H2CO3 à CO2 + H2O Type of Reaction: __________________
Octane (C8H10) is burned in oxygen gas to produce
carbon dioxide and gaseous water
______ + _______ à _______ + ________ Type of Reaction: _________________
Answer:
the answer is like same we do last I know the answer I will help you to get more questionable and paste it to you do you know what time you do it me william and paste Now bro hurry up please and then let's go play with me again Go to bed ️ I don't know what to do patch right Now or just a question for you to get more questionable
There is a certain chemical logic to the steps of the citric acid cycle. One particular functional group plays a large role in facilitating most of the chemistry that goes on in the reactions. This group is electron withdrawing, which helps to stabilize carbanion intermediates and increase the reactivity of the methyl group of acetyl CoA. What is this functional group
Answer:
Carbonyl Groups
Explanation:
Electron-withdrawing substituents stabilize the carbon atoms in its surrounding. These chemical groups are Carbonyl groups which withdraw electrons because of the inductive effect and presence of double bond between C and O and also because of the polarity of the two atoms (Carbon and oxygen)
0.41g of neon is held in a 200. mL container at 11 °C. Calculate the pressure in atm.
Answer:
2.39 atm
Explanation:
We'll begin by calculating the number of mole in 0.41 g of neon (Ne). This can be obtained as follow:
Mass of Ne = 0.41 g
Molar mass of Ne = 20 g/mol
Mole of Ne =.?
Mole = mass / molar mass
Mole of Ne = 0.41 / 20
Mole of Ne = 0.0205 mole
Next we shall convert 200 mL to L.
1000 mL = 1 L
Therefore,
200 mL = 200 mL × 1 L / 1000 mL
200 mL = 0.2 L
Next, we shall convert 11 °C to Kelvin temperature.
T(K) = T(°C) + 273
T(°C) = 11 °C
T(K) = 11 + 273
T (K) = 284 K
Finally, we shall determine the pressure. This can be obtained as follow:
Mole of Ne (n) = 0.0205 mole
Volume (V) = 0.2 L
Temperature (T) = 284 K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure (P) =?
PV = nRT
P × 0.2 = 0.0205 × 0.0821 × 284
P × 0.2 = 0.4779862
Divide both side by 0.2
P = 0.4779862 / 0.2
P = 2.49 atm
Therefore, the pressure of the gas is 2.39 atm
-4. A student learns that all of the particles within an object possess kinetic energy. Based on this fact,
the student can conclude that all of the particles in the object-
A. Contains the same atoms. B. Are hotter than their surroundings C.Are in motion. D. Are covalently bonded
Answer:
C
Explanation:
The correct option is option C. which is "are in motion".
All the particles inside an object have kinetic energy, which implies that the particles are moving. Kinetic energy is the force that drives an object's or its constituent parts in motion. As a result, it can be inferred from this fact that the object's particles are in motion.
Options A, B, and D are not necessarily true based on the given information. The fact that particles have kinetic energy does not imply that they contain the same atoms (option A), are hotter than their surroundings (option B), or are covalently bonded (option D). These characteristics are not directly related to the presence of kinetic energy in particles.
Therefore, option c is the correct option.
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Calculate mL (4 sf) of 0.7500 M sodium hydroxide required to neutralize 35.00 mL of 0.7500 M phosphoric acid. Please input number as whole number not scientific notation
Answer:
105mL of 0.7500M of NaOH are required
Explanation:
Phosphoric acid, H₃PO₄, reacts with sodium hydroxide, NaOH, as follows:
H₃PO₄ + 3 NaOH → Na₃PO₄ + 3H₂O
Where 1 mole of phosphoric acid reacts with 3 moles of NaOH
To solve this question we must find, as first, the moles of H3PO4 that react. Using the chemical equation we can find the moles of NaOH required to neutralize this acid. And, with its concentration, we can find the volume oof NaOH required:
Moles H3PO4:
35.00mL = 0.03500L * (0.7500mol / L) = 0.2625 moles H3PO4
Moles NaOH:
0.2625 moles H3PO4 * (3mol NaOH / 1mol H3PO4) = 0.07875 moles NaOH
Volume NaOH:
0.07875 moles NaOH * (1L / 0.7500mol) = 0.105L =
105mL of 0.7500M of NaOH are requiredA student pours 10.0 g of salt into a container of water and observes the amount of time it takes for the salt to dissolve. She then repeats the process using the same amounts of salt and water but this time she slowly stirs the mixture while it is dissolving. The student performs the experiment one more time but this time she stirs the mixture rapidly.
Answer:
It will go faster each time because she is stirring therefore the water can get to the salt faster than it just sitting at the top
Explanation:
A weather balloon has a volume of 105L at 0.97 atm when the temperature is 318K. What is the volume
at 293K and 1.05 atm?
Answer:
89 L
Explanation:
Step 1: Given data
Initial pressure (P₁): 0.97 atmInitial volume (V₁): 105 LInitial temperature (T₁): 318 KFinal pressure (P₂): 1.05 atmFinal volume (V₂): ?Final temperature (T₂): 293 KStep 2: Calculate the final volume of the weather balloon
If we assume that the gas inside the balloon behaves as an ideal gas, we can calculate the final volume of the gas using the combined gas law.
P₁ × V₁ / T₁ = P₂ × V₂ / T₂
V₂ = P₁ × V₁ × T₂ / T₁ × P₂
V₂ = 0.97 atm × 105 L × 293 K / 318 K × 1.05 atm = 89 L
What does the cell theory state? Answer F All organisms are composed of a nucleus G All prokaryotes are composed of multiple cells H All prokaryotes are single celled organisms J All organisms are composed of cells
Answer:
(J) All organisms are composed of cells
A saturated solution of sucrose in 500.0 mL of boiling water is cooled to 20.0 0C. What mass of rock candy will be formed?
Answer:
1280.5g
Explanation:
Would you rather
Eat sweet foods for the rest of you're life?
or
Eat salty foods for the rest of you're life?
Answer:
Salty
Explanation:
Becuase sugar isn't good for you. Unless the sweet foods are fruits but like deserted aren't good for you
Answer:
Salty
Explanation:
Too sweet foods would just crush you, but with salt at least you can drink water :)
If we have 0.06 moles of HCI
How many grams of magnesium metal is that?
Answer:
1.44 g
Explanation:
From the question given above, the following data were obtained:
Number of mole of HCl = 0.06 mole
Mass of Mg =?
From the question given above, we discovered the number of mole of HCl is equivalent to the number of mole of Mg. Thus,
Number of mole of Mg = number of mole of HCl
Number of mole of Mg = 0.06 mole
Finally, we shall determine the mass of Mg. This can be obtained as follow:
Number of mole of Mg = 0.06 mole
Molar mass of Mg = 24 g/mol
Mass of Mg =?
Mass = mole × molar mass
Mass of Mg = 0.06 × 24
Mass of Mg = 1.44 g
Therefore, the mass of magnesium is 1.44 g
A balloon is filled with 3.50 L of water at 24.0°C. What is the volume of the water at 307 K?
Answer:
what is the volume of the water at 307 k?
14. The illustration below shows two atoms of a fictitious element (M) forming a diatomic
molecule. What type of bonding occurs between these two atoms?
A. Covalent
B. Hydrogen
C. lonic
D. Polar
Covalent bonding involving covalent bonds is depicted between these two atoms as they form diatomic molecule.
What is a covalent bond?Covalent bond is defined as a type of bond which is formed by the mutual sharing of electrons to form electron pairs between the two atoms.These electron pairs are called as bonding pairs or shared pair of electrons.
Due to the sharing of valence electrons , the atoms are able to achieve a stable electronic configuration . Covalent bonding involves many types of interactions like σ bonding,π bonding ,metal-to-metal bonding ,etc.
Sigma bonds are the strongest covalent bonds while the pi bonds are weaker covalent bonds .Covalent bonds are affected by electronegativities of the atoms present in the molecules.Compounds having covalent bonds have lower melting points as compared to those with ionic bonds.
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