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Stoichiometry

CH 4g + 2O ...

Question

CH $_{4}$ (g) + 2O $_{2}$ (g) $\to$ CO $_{2}$ (g) + 2H $_{2}$ O(g) + 800 kJ
Find the energy produced in above reaction, if 1 mole of $O_{2}$ (g) is consumed.

200 kJ

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400 kJ

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800 kJ

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1,200 kJ

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1,600 kJ

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Solution

The correct option is B 400 kJ
When 2 moles of oxygen is consumed, the energy produced is 800 kJ.
When 1 mole of oxygen is consumed, the energy produced is 400 kJ.

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Similar questions

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g) + 800 k J

O_{2} (g)

Calculate the heat of combustion (in KJ) of

methane from the following data

i) C (graphite) + 2H $_{2}$ (g) $\to$ CH $_{4}$ (g), $Δ$ H = -74.8 kJ

ii) C (graphite) + O $_{2}$ (g) $\to$ CO $_{2}$ (g), $Δ$ H = -393.5 kJ

iii) H $_{2}$ (g) +1/2O $_{2}$ (g) $\to$ H $_{2}$ O $(l)$ , $Δ$ H = -286.2 KJ.

H_{2}

C H_{4} (g) + \frac{1}{2} O_{2} (g) \to C O (g) + 2 H_{2} (g)

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (g); △ H = - 800 k J

C H_{4} (g) + C O_{2} (g) \to 2 C O (g) + 2 H_{2} (g); △ H = + 235 k J

C H_{4} (g) + H_{2} O (g) \to C O (g) + 3 H_{2} (g); △ H = + 204 k J

△ H

C O (g) + {2 H}_{2} (g) ⇄ {C H}_{3} O H (g); Δ_{f} H^{o} = - 92.0 k J / m o l

Calculate the standard internal energy change for the reaction at 25⁰C:-

C₂H₄(g) + 3O₂(g)----------à 2CO₂ (g) + 2H₂O (l) DH for C₂H₄ (g) = 52.30 kJ/mole,

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