Which equation shows conservation of atoms?A) H2 + O 2 --> H2O
B) H2 + O 2 --> 2H2O
C) 2H2 + O2 --> 2H2O
D) 2H2 + 2O2 --> 2H2O

Answers

Answer 1

Answer:

Answer: The equation showing conservation of atoms is $2H_2+O_2\rightarrow H_2O$

Explanation:

Every balanced chemical equation follows law of conservation of mass.

This law states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form. This also means that total number of individual atoms on reactant side must be equal to the total number of individual atoms on the product side.

For the given chemical equations:

Option A:

The given chemical equation follows:

$H_2+O_2\rightarrow H_2O$

There are 2 hydrogen atoms and 2 oxygen atoms on the reactant side and 2 hydrogen and 1 oxygen atom on product side.

So, this equation does not show conservation of atoms.

Option B:

The given chemical equation follows:

$H_2+O_2\rightarrow 2H_2O$

There are 2 hydrogen atoms and 2 oxygen atoms on the reactant side and 4 hydrogen atoms and 2 oxygen atoms on product side.

So, this equation does not show conservation of atoms.

Option C:

The given chemical equation follows:

$2H_2+O_2\rightarrow H_2O$

There are 4 hydrogen atoms and 2 oxygen atoms on the reactant side and 4 hydrogen atoms and 2 oxygen atoms on product side.

So, this equation shows conservation of atoms.

Option D:

The given chemical equation follows:

$2H_2+2O_2\rightarrow 2H_2O$

There are 4 hydrogen atoms and 4 oxygen atoms on the reactant side and 4 hydrogen atoms and 2 oxygen atoms on product side.

So, this equation does not show conservation of atoms.

Hence, the equation showing conservation of atoms is $2H_2+O_2\rightarrow H_2O$

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Given the balanced equation representing a reaction:CH4(g) + 2O2(g) --> 2H2O(g) + CO2(g) + heatWhich statement is true about energy in this reaction?(1) The reaction is exothermic because it releases heat.(2) The reaction is exothermic because it absorbs heat.(3) The reaction is endothermic because it releases heat.(4) The reaction is endothermic because it absorbs heat.

The maximum energy available for useful work from a spontaneous reaction(A) free energy
(B) lattice energy
(C) kinetic energy
(D) activation energy
(E) ionization energy

Answers

The answer is: A; Free Energy

Is CI3 a compound or an element

Answers

Cl₃ is formed by thecombination of 3 chlorine atoms. Hence, not a single element and not a compound. Instead Cl₃ is a molecule of chlorine.

What are molecules ?

Molecules are the combination of atoms of same element or are the basic units of a compound. A compound is formed by the combination of two or more atoms of different elements.

The combination of atoms can be different bond types, such as ionic bond, covalent bond, hydrogen bonding etc. The type of bond is dependent on the nature of atoms.

Combination of same atoms in any number are forming the molecules of that element and not a compound. Hence, Cl₃ is a molecules and not element or compound.

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Answer:

CI3 is a compound called carbon tetra iodide

The complete combustion of ethanol, C₂H₅OH (FW = 46.0 g/mol), proceeds as follows: $C_2H_5OH(l) + 3O_2(g) \rightarrow 2CO_2(g) + 3H_2O(l)$ ; ΔH = −555 kJ What is the enthalpy change for combustion of 15.0 g of ethanol?

Answers

Answer: 181 kJ

Explanation:

The balanced chemical reaction is;

$C_2H_5OH(l)+3O_2(g)\rightarrow 2CO_2(g)+3H_2Ol)$ $\Delta H=-555jJ$

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=(15.0g)/(46.0g/mol)=0.326moles$

According to stoichiometry:

1 mole of $C_2H_5OH$ on complete combustion give= 555 kJ

Thus 0.326 moles of $C_2H_5OH$ on complete combustion give= $(555)/(1)* 0.326=181kJ$

Thus the enthalpy change for combustion of 15.0 g of ethanol is 181 kJ

Calculate the mass of water produced when 2.06 g of butane reacts with excess oxygen.

Answers

2C4H10 + 13O2 = 8CO2 + 10H2O

1. (2.06g C4H10)/(58.12 g/mol C4H10) = 0.035mol C4H10

2. (0.035molC4H10)(10 mol H2O/2mol C4H10) = 0.177mol H2O

3. (0.177mol H2O)(18.01g/mol H2O) = 3.19g H2O

In comparison with liquids and gases, solids area. more dense.
b. more easily compressed.
c. less organized.
d. more likely to flow.

Answers

In comparison with liquids and gases, solids are more dense. The answer is letter B. The solid has a more definite shape and volume. The particles are locked into place. It cannot be further compressed due to the bond that exists between the molecules. The kinetic energy of the molecules is close to none because the molecules are so close and so compact with each other.

Carbon dioxide is a green house gas that is linked to global warming. It is released into the atmosphere through the combustion of octane (C8H18) in gasoline. Write the balanced chemical equation for the combustion of octane. (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.)Calculate the mass of octane needed to release 3.50 mol CO2.

Answers

Final answer:

The balanced chemical equation for the combustion of octane is 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O. From the stoichiometry of the reaction, 3.50 mol of CO2 will need approximately 50g of octane.

Explanation:

The combustion of octane (C8H18) in the presence of oxygen (O2) produces carbon dioxide (CO2) and water (H2O). The balanced chemical equation for this reaction is: 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O.

To calculate the mass of octane needed to release 3.50 mol CO2, we need to understand the stoichiometry of the reaction. From the balanced equation, we can see that 16 mol of CO2 is produced from 2 mol of C8H18. So, 1 mol of C8H18 produces 8 mol of CO2.

Therefore, to produce 3.50 mol of CO2, we would need 3.50/8 = 0.4375 mol of C8H18. The molar mass of octane is approximately 114 g/mol, so the required mass would be 0.4375mol x 114g/mol = approximately 50g.

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Final answer:

The combustion of octane produces carbon dioxide and water, as described by the balanced chemical equation C8H18 + 12.5O2 → 8CO2 + 9H2O. To produce 3.50 mol of CO2, approximately 50g of octane is needed.

Explanation:

The combustion of octane (C8H18) in the presence of oxygen (O2) produces carbon dioxide (CO2) and water (H2O). The balanced chemical equation for this reaction is: C8H18 + 12.5O2 → 8CO2 + 9H2O.

Considering the stoichiometry of the reaction, we can see that 1 mol of octane produces 8 moles of CO2. Therefore, to produce 3.50 mol of CO2, the amount of octane required would be 3.50/8 = 0.4375 mol. Converting this to mass using the molar mass of octane (114.22 g/mol), we get 0.4375 mol * 114.22 g/mol ≈ 50 g. Thus, approximately 50g of octane is needed to produce 3.50 mol of CO2.