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Standard XII

Chemistry

Heat of Reaction

Consider the ...

Question

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

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
In eqn (i), no bond is being broken while in eqn (ii), 2 H - H bonds are broken. So, in eqn (ii) some of the energy is used up to break the bonds.

Thus, x > y.

Suggest Corrections

Similar questions

Q. Consider the reactions given below. on the basis of these reactions find out which of the algebric relation given in options (i) to (iv) is correct ? (i)

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

m o l^{- 1}

(ii)

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}

Q. 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}

Q. Given,

C_{(g r a p h i t e s)} + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l);

Δ_{r} H^{\circ} = - 285.8 k J m o l^{- 2}

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

Δ_{r} H^{\circ} = + 890.3 k J m o l^{- 1}

Based on the above thermochemical equations, the value of

Δ_{r} H^{\circ}

at 298K for the reaction,

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

will be

Consider the reactions given below. On the basis of these reactions find out which of the algebraic relationship given in options (a) to (d) is correct?
$1. C (g) + 4 H (g) \to C H_{4} (g); Δ_{r} H = x k J m o l^{- 1} 2. C (g r a p h i t e) + 2 h_{2} (g) \to C H_{4} (g); Δ_{r} H = y k J m o l^{- 1}$
(a) x = y
(b) x = 2y
(c) x > y
(d) x < y

Q. Given,

C_{(g r a p h i t e s)} + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l);

Δ_{r} H^{\circ} = - 285.8 k J m o l^{- 2}

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

Δ_{r} H^{\circ} = + 890.3 k J m o l^{- 1}

Based on the above thermochemical equations, the value of

Δ_{r} H^{\circ}

at 298K for the reaction,

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

will be

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Consider the reaction given below. On the basis of these reactions find out which of the algebraic relations given in options (A) to (D) is correct?(i) C(g)+4H(g)→CH4(g);ΔrH=xkJmol−1(ii) C(graphite,s)+2H2(g)→CH4(g);ΔrH=ykJmol−1

The correct option is C x > yIn eqn (i), no bond is being broken while in eqn (ii), 2 H - H bonds are broken. So, in eqn (ii) some of the energy is used up to break the bonds. Thus, x > y.

The correct option is C x > y
In eqn (i), no bond is being broken while in eqn (ii), 2 H - H bonds are broken. So, in eqn (ii) some of the energy is used up to break the bonds.

Thus, x > y.