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Molar and Specific Heat Capacity

The standard ...

Question

The standard enthalpy of formation of propene, $C_{3} H_{6}$ is $+ 20.6 k J / m o l e$ . Calculate the heat of combustion of one mole of $C_{3} H_{6}$ . The heats of formation of $C O_{2} (g)$ and $H_{2} O (l)$ are $- 394 k J / m o l e$ and $- 285.8 k J / m o l e$
[Give your answer in terms of magnitude of the heat of combustion]

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Solution

$C_{3} H_{6} + \frac{9}{2} O_{2} ⟶ 3 C O_{2} + 3 H_{2} O$

$3 C + 3 H_{2} ⟶ C_{3} H_{6} Δ H = + 20.6 k J / m o l e$

$C + O_{2} ⟶ C O_{2} Δ H = - 394 k J / m o l e$

$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O Δ H = - 285.8 k J / m o l e$

${(Δ H_{C})}_{C_{3} H_{6}} = [3 Δ H_{C O_{2}} + 3 Δ H_{f (H_{2} O)} - Δ H_{f (C_{3} H_{6})}]$

$= [3 \times (- 394) + 3 (- 285.8) - 20.6]$

${(Δ H_{C})}_{C_{3} H_{6}} = - 2060 k J / m o l e$

$| {(Δ H_{C})}_{C_{3} H_{6}} | = | - 2060 | = 2060$

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Similar questions

Q. The standard enthalpy of formation of propene,

C_{3} H_{6}

is +20.6 kJ mol

^{- 1}

. The heats of formation of

C O_{2} (g)

H_{2} O (l)

are -394 kJ mol

^{- 1}

. and -285.8 kJ mol

^{- 1}

Calculate the heat of combustion of one mole of

C_{3} H_{6}

.

Q. The heats of formation of

C O_{2} (g)

H_{2} O (l)

- 394 k J / m o l e

- 285.8 k J / m o l e

respectively. Using the data for the following combustion reaction, calculate the heat of formation of

C_{3} H_{8} (g)

.

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

Δ H^{\circ} = - 2221.6 k J

.

Q. The combustion of one mole of benzene takes place at 298K and 1 atm after combustion

C O_{2 (g)}

H_{2} O_{J}

are produced and 3267.0 KJ of heat is liberated. Calculate the standard enthalpy of formulation

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of benzene. Standard enthalpy of formation of

C O_{2 (g)}

H_{2} O_{J}

are -393.5Kj and -285.83Kl/Mole

2

C_{2} H_{6}

are completely burnt,

3120 k J

of heat is liberated. Calculate the heat of formation

Δ H_{f}^{o}

C_{2} H_{6}

Δ H_{f}^{o}

{C O}_{2} (g)

H_{2} O (l)

- 395

- 286 k J

Q. The heats of formation of

C O_{2} (g)

H_{2} O (l)

- 394

- 285.8

kJ/mole respectively. Using the data for the following combustion reaction, calculate the heat of formation of

C_{2} H_{2} (g)

.

2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 C O_{2} (g) + 2 H_{2} O (l)

Δ H^{o} = - 2601

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