Answers Chemistry Credit Recovery BEnthalpy of Reaction

Lab: Enthalpy Answers

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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).

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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.

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.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).

Consider the following intermediate chemical equations.What is the enthalpy of the overall chemical equation NO(g) + O(g) NO(g)?

-305 kJ

-304.1 kJ

-93.7 kJ

588.7 kJ

When two intermediate chemical equations are combined, the same substance that appears in the same phase can be canceled out, provided that

it is a reactant in one intermediate reaction and a catalyst in the other reaction.

it is a product in one intermediate reaction and a catalyst in the other reaction.

it is a reactant in one intermediate reaction and a product in the other reaction.

it is a reactant in both of the intermediate reactions.

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.

Consider the intermediate chemical reactions.The final overall chemical equation is . When the enthalpy of this overall chemical equation is calculated, the enthalpy of the second intermediate equation