The heats of combustion of $C H_{4} & C_{4} H_{10}$ are -890.3 $k J m o l^{- 1} & - 2878.7 k J m o l^{- 1}$ respectively. Which of the two has greater efficiency as fuel per gram?

Methane

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Butane

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Solution

The correct option is A
Methane

Molar mass of methane = 16

Molar mass of butane = 58

Heat produced per gram of methane = $\frac{- 890.3}{16}$

= -55.64kJ

Heat produced per gram of butane = $\frac{12878.7}{58}$ = -49.63 kJ

$∴$ Methane has greater fuel efficiency.

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The heats of combustion of CH4 & C4H10 are -890.3 kJ mol−1 & −2878.7 kJ mol−1 respectively. Which of the two has greater efficiency as fuel per gram?

The correct option is A Methane Molar mass of methane = 16 Molar mass of butane = 58 Heat produced per gram of methane =−890.316 = -55.64kJ Heat produced per gram of butane = 12878.758 = -49.63 kJ ∴ Methane has greater fuel efficiency.

The heats of combustion of $C H_{4} & C_{4} H_{10}$ are -890.3 $k J m o l^{- 1} & - 2878.7 k J m o l^{- 1}$ respectively. Which of the two has greater efficiency as fuel per gram?

The correct option is A
Methane

Molar mass of methane = 16

Molar mass of butane = 58

Heat produced per gram of methane = $\frac{- 890.3}{16}$

= -55.64kJ

Heat produced per gram of butane = $\frac{12878.7}{58}$ = -49.63 kJ

$∴$ Methane has greater fuel efficiency.