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Enthalpy of Reaction Answers

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How should the enthalpy of an intermediate step be manipulated when used to produce an overall chemical equation?

Multiply the enthalpy by 1 if the chemical equation is reversed.

Multiply the enthalpy by –1 if the chemical equation is reversed.

Add 2 to the enthalpy if the coefficients must be doubled.

Add 2 to the enthalpy if the coefficients must be cut in half.

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Consider the following intermediate chemical equations.Which overall chemical equation is obtained by combining these intermediate equations?

Upper C upper H subscript 4 plus 2 upper O subscript 2 (g) right arrow upper C upper O subscript 2 (g) plus 2 upper H subscript 2 upper O (l).

Upper C upper H subscript 4 plus 2 upper O subscript 2 (g) right arrow upper C upper O subscript 2 (g) plus 2 upper H subscript 2 upper O (g).

Upper C upper H subscript 4 plus 2 upper O subscript 2 (g) right arrow upper C upper O subscript 2 (g) plus 4 upper H subscript 2 upper O (g) plus 2 upper H subscript 2 upper O (l).

Upper C upper H subscript 4 plus 2 upper O subscript 2 (g) right arrow upper C upper O subscript 2 (g) plus 6 upper H subscript 2 upper O (g).

Jason combines the two intermediate steps shown.Which best describes what Jason should do with the oxygen molecules?

Place two of them as products.

Place two of them as reactants.

Cancel them out because there is one in each equation.

Double them because there is one in each equation.

Consider the following intermediate chemical equations.In the final chemical equation, HF and O are the products that are formed through the reaction between and F. Before you can add these intermediate chemical equations, you need to alter them by multiplying the

second equation by 2 and reversing the first equation.

first equation by 2 and reversing it.

first equation by (1/2) and reversing the second equation.

second equation by 2 and reversing it.

Consider the following intermediate chemical equations.What is the enthalpy of the overall chemical reaction ?

-205.7 kJ

-113.4 kJ

-14.3 kJ

78.0 kJ

What is enthalpy?

the total concentration of the system

the total heat content of the system

the total pressure of the system

the total disorder of the system

Consider the following intermediate chemical equations.In the final chemical equation, NaCl and O are the products that are formed through the reaction between and Cl. Before you can add these intermediate chemical equations, you need to alter them by

multiplying the second equation by 2.

multiplying the first equation by 2.

multiplying the first equation by (1/2).

multiplying the second equation by (1/4).

Consider the following enthalpy diagram.What is the overall enthalpy change DHrxn for the system?

-1,300 kJ

-300 kJ

300 kJ

1,300 kJ

What is the final chemical equation from the following intermediate chemical equations?

Upper P subscript 4 upper O subscript 6 (s) plus 2 upper O subscript 2 (g) right arrow upper P subscript 4 upper O subscript 10 (s).

Upper P subscript 4 upper O subscript 6 (s) plus 8 upper O subscript 2 (g) right arrow 2 upper P subscript 4 (s) plus upper P subscript 4 upper O subscript 10 (s).

Upper P subscript 4 upper O subscript 6 (s) plus 15 upper O subscript 2 (g) right arrow upper P subscript 4 (s) plus upper P subscript 4 upper O subscript 10 (s).

Upper P subscript 4 upper O subscript 6 (s) StartFraction 5 over 3 EndFraction upper O subscript 2 (g) right arrow upper P subscript 4 upper O subscript 10 (s).

If a chemical reaction is reversed, what happens to the enthalpy of the reaction?

The enthalpy of the reaction becomes zero.

The enthalpy of the reaction doubles.

The sign of the enthalpy of the reaction reverses.

The enthalpy of the reaction is halved.

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Enthalpy of Reaction Answers

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