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The standard enthalpy of formation of propene, $C_{3} H_{6}$ , is $+ 20.6 kJ / mole$ . Calculate the heat of combustion of one mole of $C_{3} H_{6}$ . The heats of formation of ${CO}_{2} (g)$ and $H_{2} O (l)$ are $- 394 kJ / mole$ and $- 285.8 kJ / mole$ respectively.

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Important Questions on Thermodynamics

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 17

The fat, glyceryl trioleate, is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy $(kJ)$ liberated when $1.00 g$ of this fat reacts.

(Atomic weights: $C = 12.01, H = 1.008, O = 16.00$ )

$C_{57} H_{107} O_{6} (s) + 80 O_{2} (g) \to 57 {CO}_{2} + 52 H_{2} O (l)$

$∆ H ° C_{57} H_{107} O_{6} = - 70870 kJ / mole$

$∆ H ° H_{2} O (l) = - 285.8 kJ / mole$

$∆ H ° {CO}_{2} (g) = - 393.5 kJ / mole$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 18

Using the enthalpies of formation, calculate the energy $(kJ)$ released when $3.00 g$ of ${NH}_{3 (g)}$ reacts according to the following equation.

(Atomic weights: $B =10.81, O =16.00, H =1.008$ )

$4 {NH}_{3} (g) + 5 O_{2} (g) \to 4 NO (g) + 6 H_{2} O (g)$

$∆ H ° {NH}_{3} (g) = - 46.1 kJ / mole$

$∆ H ° NO (g) = + 90.2 kJ / mole$

$∆ H ° H_{2} O (g) = - 241.8 kJ / mole$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 19

A sheet of

15.0 g

of gold at

25.0 ° C

is placed on a

30.0 g

sheet of copper at

45.0 ° C

. What is the final temperature of the two metals assuming that no heat is lost to the surroundings. The specific heats of gold and copper are

0.129 J / g ° C

and

0.385 J / g ° C

respectively.

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 20

Calculate the heat of combustion $(kJ)$ of propane, $C_{3} H_{8}$ using the listed standard enthalpy of reaction data:

$C_{3} H_{8} (g) + 5 O_{2} (g) \to 3 {CO}_{2} (g) + 4 H_{2} O (g)$

$3 C (s) + 4 H_{2} (g) \to C_{3} H_{8} (g)$ $∆ H ° / KJ = - 103.8$

$C (s) + O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / KJ = - 393.5$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (g)$ $∆ H ° / KJ = - 241.8$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 21

Calculate the value of $∆ H ° / kJ$ for the following reaction using the listed thermochemical equations:

$2 C (s) + H_{2} (g) \to C_{2} H_{2} (g)$

$2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 {CO}_{2} (g) + 2 H_{2} O (l)$ $∆ H ° / kJ = - 2600 kJ$

$C (s) + O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / kJ = - 390 kJ$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ $∆ H ° / kJ = - 572 kJ$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 22

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

$C_{2} H_{5} OH (l) + 3 O_{2} (g) \to 2 {CO}_{2} (g) + 3 H_{2} O (g)$

$∆ H_{f}^{°} C_{2} H_{5} OH (l) = - 277.7 kJ / mole$

$∆ H_{f}^{°} {CO}_{2} (g) = - 393.5 kJ / mol$

$∆ H_{f}^{°} H_{2} O (g) = - 241.8 kJ / mole$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 23

Calculate $∆ H ° / kJ$ for the following reaction using the listed standard enthalpy of reaction data:

$2 N_{2} (g) + 5 O_{2} (g) \to 2 N_{2} O_{5} (s)$

$N_{2} (g) + 3 O_{2} (g) + H_{2} (g) \to 2 {HNO}_{3} (aq)$ $∆ H ° / kJ = - 414.0$

$N_{2} (g) + 3 O_{2} (g) + H_{2} (g) \to 2 {HNO}_{3} (aq)$ $∆ H ° / kJ = - 86.0$

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ $∆ H ° / kJ = - 571.6$

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 24

Determine $∆ H ° / kJ$ for the following reaction using the listed enthalpies of reaction:

$4 CO (g) + 8 H_{2} (g) \to 3 {CH}_{4} (g) + {CO}_{2} (g) + 2 H_{2} O (l)$

$C (graphite) + \frac{1}{2} O_{2} (g) \to CO (g)$ $∆ H ° / kJ = - 110.5 kJ$

$CO (g) + \frac{1}{2} O_{2} (g) \to {CO}_{2} (g)$ $∆ H ° / kJ = - 282.9 kJ$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$ $∆ H ° / kJ = - 285.8 kJ$

$C (graphite) + 2 H_{2} (g) \to {CH}_{4} (g)$ $∆ H ° / kJ = - 74.8 kJ$

The standard enthalpy of formation of propene, C3H6, is +20.6 kJ/mole. Calculate the heat of combustion of one mole of C3H6. The heats of formation of CO2g and H2Ol are -394 kJ/mole and -285.8 kJ/mole respectively.

Important Questions on Thermodynamics

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The standard enthalpy of formation of propene, $C_{3} H_{6}$ , is $+ 20.6 kJ / mole$ . Calculate the heat of combustion of one mole of $C_{3} H_{6}$ . The heats of formation of ${CO}_{2} (g)$ and $H_{2} O (l)$ are $- 394 kJ / mole$ and $- 285.8 kJ / mole$ respectively.