Consider the reactions given below. On the basis of these reactions find out which of the following relations is correct?
$(i) C_{(g)} + 4 H_{(g)} \to C H_{4 (g)}; △_{r} H = x k J m o l^{- 1} (i i) C (g r a p h i t e, s) + 2 H_{2 (g)} \to C H_{4 (g)}; △_{r} H = y k J m o l^{- 1}$

x = y

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x = 2y

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x > y

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x < y

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Solution

The correct option is C x > y
Same bonds are formed in reactions (i) and (ii) but no bonds are broken in reaction (i) whereas bonds in the reactant molecules are broken in reaction (ii). As energy is absorbed when bonds are broken, energy released in reaction (i) is greater than that in reaction (ii), i.e., x > y.

Suggest Corrections

Similar questions

C (g) + 4 H (g) \to C H_{4} (g); Δ H = x k J

m o l^{- 1}

C (g r a p h i t e) + 2 H_{2} (g) \to C H_{4} (g); Δ H = y k J

m o l^{- 1}

C_{(g)} + 4 H_{(g)} \to C H_{4 (g)}; Δ_{r} H = x k J m o l^{- 1}

C_{(g r a p h i t e, s)} + 2 H_{2 (g)} \to C H_{4 (g)}; Δ_{r} H = y k J m o l^{- 1}

C (s) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H = - X k c a l

C (g) + 4 H (g) ⟶ C H_{4} (g); Δ H = - X_{1} k c a l

C H_{4} (g) ⟶ C H_{3} (g) + H (g); Δ H = + Y k c a l

C - H

(i) C_{(g)} + 4 H_{(g)} \to C H_{4 (g)}; △_{r} H = x k J m o l^{- 1} (i i) C (g r a p h i t e, s) + 2 H_{2 (g)} \to C H_{4 (g)}; △_{r} H = y k J m o l^{- 1}

C (d i a m o n d) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H_{1}

C (g) + 4 H (g) ⟶ C H_{4} (g); Δ H_{2}

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