Question 1

Given the reaction

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

, calculate the enthalpy change (

\Delta H

) using the following bond energies:

H-H = 436 	ext{ kJ/mol}

,

Cl-Cl = 243 	ext{ kJ/mol}

, and

H-Cl = 432 	ext{ kJ/mol}

.

Accepted Answer

-185 kJ/mol

Answer

-247 kJ/mol

Answer

+247 kJ/mol

Answer

+185 kJ/mol

Question 2

Calculate the enthalpy change (

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

) for the combustion of methane:

\Delta H

. Use these average bond energies:

H-H = 436 	ext{ kJ/mol}

,

Cl-Cl = 243 	ext{ kJ/mol}

,

H-Cl = 432 	ext{ kJ/mol}

, and

O-H = 464 	ext{ kJ/mol}

.

Accepted Answer

-808 kJ/mol

Answer

-612 kJ/mol

Answer

-1042 kJ/mol

Answer

+818 kJ/mol

Question 3

The decomposition of nitrogen trichloride is given by the equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Given the bond energies

\Delta H

,

H-H = 436 	ext{ kJ/mol}

, and

Cl-Cl = 243 	ext{ kJ/mol}

, calculate the enthalpy change (

H-Cl = 432 	ext{ kJ/mol}

) for the reaction.

Accepted Answer

-470 kJ/mol

Answer

+470 kJ/mol

Answer

-270 kJ/mol

Answer

+270 kJ/mol

Question 4

The formation of ammonia is represented by the equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Given the bond energies

\Delta H

,

H-H = 436 	ext{ kJ/mol}

, and

Cl-Cl = 243 	ext{ kJ/mol}

, calculate the enthalpy change (

H-Cl = 432 	ext{ kJ/mol}

) for the reaction.

Accepted Answer

-97 kJ/mol

Answer

-84 kJ/mol

Answer

+97 kJ/mol

Answer

-1095 kJ/mol

Question 5

The combustion of hydrazine is represented by the equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Using the bond energies

\Delta H

,

H-H = 436 	ext{ kJ/mol}

,

Cl-Cl = 243 	ext{ kJ/mol}

,

H-Cl = 432 	ext{ kJ/mol}

, and

O-H = 464 	ext{ kJ/mol}

, calculate the enthalpy change (

\Delta H

) for this reaction.

Accepted Answer

-571 kJ/mol

Answer

-1167 kJ/mol

Answer

-783 kJ/mol

Answer

+571 kJ/mol

Question 6

The synthesis of hydrogen fluoride is represented by the equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Given the bond energies

\Delta H

,

H-H = 436 	ext{ kJ/mol}

, and the enthalpy change for the reaction is

Cl-Cl = 243 	ext{ kJ/mol}

, calculate the bond energy of the

H-Cl = 432 	ext{ kJ/mol}

bond.

Accepted Answer

568 kJ/mol

Answer

284 kJ/mol

Answer

516 kJ/mol

Answer

1136 kJ/mol

Question 7

The combustion of methanol occurs according to the following equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Given the bond energies

\Delta H

,

H-H = 436 	ext{ kJ/mol}

,

Cl-Cl = 243 	ext{ kJ/mol}

,

H-Cl = 432 	ext{ kJ/mol}

,

O-H = 464 	ext{ kJ/mol}

, calculate the enthalpy change (

\Delta H

) for the reaction.

Accepted Answer

-1274 kJ/mol

Answer

-1452 kJ/mol

Answer

+1274 kJ/mol

Answer

-637 kJ/mol

Question 8

The chemical reaction for the formation of hydrogen iodide is

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Given the bond energies:

\Delta H

,

H-H = 436 	ext{ kJ/mol}

, and

Cl-Cl = 243 	ext{ kJ/mol}

, calculate the enthalpy change (

H-Cl = 432 	ext{ kJ/mol}

) for the reaction.

Accepted Answer

-11 kJ/mol

Answer

+11 kJ/mol

Answer

+288 kJ/mol

Answer

-288 kJ/mol

Question 9

The combustion of ethyne occurs according to the equation:

H_2(g) + Cl_2(g) 
ightarrow 2HCl(g)

. Using the following bond energies:

\Delta H

,

H-H = 436 	ext{ kJ/mol}

,

Cl-Cl = 243 	ext{ kJ/mol}

,

H-Cl = 432 	ext{ kJ/mol}

, and

O-H = 464 	ext{ kJ/mol}

, calculate the enthalpy change (

\Delta H

) for the reaction.

Accepted Answer

-2246 kJ/mol

Answer

-1123 kJ/mol

Answer

-1890 kJ/mol

Answer

+2246 kJ/mol

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