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What can be concluded about the value of $∆ H$ and $∆ S$ from this graph?

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Important Questions on Thermodynamics

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IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 14

For which of the following processes, total entropy of universe increases.

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 15

1

mole of an ideal gas at

25 ° C

is subjected to expand reversibly ten times of its initial volume. The change in entropy due to expansion is:

HARD

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Beta Question Bank for Engineering: Chemistry>Chapter 4 - Thermodynamics>EXERCISE-2>Q 16

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.

HARD

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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:

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

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

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

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

What can be concluded about the value of ∆H and ∆S from this graph?

Important Questions on Thermodynamics

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What can be concluded about the value of $∆ H$ and $∆ S$ from this graph?