$C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g) + 800 k J$ . If a mole of $O_{2} (g)$ is consumed in the reaction, what energy is produced?

200 k J

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400 k J

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800 k J

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1200 k J

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1600 k J

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Solution

The correct option is B $400 k J$
2 moles of $O_{2}$ consumed in above reaction then energy produced $=$ $800 k J$
so if 1 moles of $O_{2}$ consumed in above reaction then energy produced $=$ $800 / 2 k J$ $=$ $400 k J$

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Similar questions

X Y, X_{2}

Y_{2}

Δ_{f} H

X Y

- 200 kJ/mol

X_{2}

Complete and balance the following reaction:

${CH}_{4} (g) + O_{2} (g) \to$

Which of the following reactions is not correct according to the law of conservation of mass ?

(a) $2 M g (s) + O_{2} (g) \to 2 M g O (s)$

(b) $C_{3} H_{8} (g) + O_{2} (g) \to C O_{2} (g) + H_{2} O (g)$

(d) $C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g)$

Δ H

Δ U

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g); Δ H = - 890.4 k J

2 H g O (s) \to 2 H g (l) + O_{2} (g); Δ H = + 181.6 k J

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