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Limitations of First Law

What will be ...

Question

What will be the amount of heat evolved by burning $10 L$ of methane under standard conditions?
(Given heats of formation of $C H_{4}, C O_{2} a n d H_{2} O a r e - 76.2, - 398.8 a n d - 241.6 k J m o l^{- 1}$ respectively)

A

805.8 k J

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B

398.8 k J

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C

359.7 k J

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D

640.4 k J

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Solution

The correct option is C $359.7 k J$
Equation,
$C H_{4} + 2 O_{2} \to C O_{2} + 2 H_{2} O$
$Δ H = H_{P (P r o d u c t)} - H_{R (R e a c t a n t)}$
$Δ H_{f}^{\circ} (C O_{2}) + 2 Δ H_{f}^{\circ} (H_{2} O) - (Δ H_{f}^{\circ} (C H_{4}) + 2 Δ H_{f}^{\circ} (O_{2}))$
$= - 398.8 - 2 \times 241.6 - (- 76.2 + 2 \times 0) = - 805.8 k J m o l^{- 1}$
$22.4 L o f C H_{4} ( 1 mole) gives 805.8 k J$
$10 L o f C H_{4} will give \frac{805.8}{22.4} \times 10 = 359.73 k J$
Hence, Option C is correct.

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Similar questions

Q. What will be the amount of heat evolved by burning 10 L of methane under standard conditions?
(Given heats of formation of

C H_{4}, C O_{2}

H_{2} O

are -76.2, -398.8 and -241.6 kJ

m o l^{- 1}

Q. The standard heats of formation of

{C H}_{4} (g), {C O}_{2} (g)

H_{2} O (g)

- 76.2, - 398.8

- 241.6

k J {m o l}^{- 1}

respectively. Calculate the amount of heat evolved by burning

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Q. The standard heat of formation of

C H_{4 (g)}, C O_{2 (g)}

H_{2} O_{(g)}

- 76.2, - 398.8, - 241.6

k J m o l^{- 1}

respectively. the amount of heat evolved

(i n k J)

m^{3}

of methane measured under normal conditions is

Q. The standard heat of formation of

C H_{4} (g), C O_{2} (g) a n d H_{2} O (g)

are -76.2, -398.8 and -241.6

k J m o l^{- 1}

respectively. Calculate the amount of heat evolved by burning

1 m^{3}

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Q. The standard heat of formation of

C H_{4 (g)}, C O_{2 (g)}

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m^{3}

of methane measured under normal conditions is

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