Heat of React...

Heat of Reaction

Trending Questions

Q. Consider the reactions

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

The average bond energy of

C - H

bond in methane is

$\frac{x}{4} k c a l m o l^{- 1}$
$x_{1} k c a l m o l^{- 1}$
$\frac{x_{1}}{4} k c a l m o l^{- 1}$
$y k c a l m o l^{- 1}$

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Q. Heat produced in calories by the combustion of one gram of carbon is called

Heat of combustion of carbon
Heat of formation of carbon
Calorific value of carbon
Heat of production of carbon

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Consider the following data:

$Δ f H^{0} (N_{2} H_{4}, l) = 50 k J / m o l$

$Δ f H^{0} (N H_{3}, g) = - 46 k J / m o l$

$B . E . (N - H) = 393 k J / m o l$ and $B . E . (H - H) = 436 k J / m o l$ , also $Δ_{v a p} H (N_{2} H_{4}, l) = 18 k J / m o l$

The N- N bond energy in $N_{2} H_{4}$ is

226 kJ/mol
154 kJ/mol
190 kJ/mol
45.45 kJ/mol

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Q. If the heat of dissolution of

a n . C u S O_{4}

and

C u S O_{4} .5 H_{2} O

are (-15.89) kcal and 2.80 kcal respectively. Calculate the heat of hydration of

C u S O_{4}

18.69 kcal
-13.09 kcal
-18.69 kcal
13.09 kcal

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Q. The heats of combustion of rhombic and monoclinic sulphur are 70960 and 71030 cal/mol respectively. Calculate the heat of conversion of rhombic to monoclinic sulphur

70960 cal
- 70 cal
71030 cal
70 cal

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Q. The enthalpy of solution of

B a C l_{2} (s)

and

B a C l_{2} .2 H_{2} O (s)

are – 20.6 and 8.8 kJ

m o l^{- 1}

respectively, the enthalpy change for the hydration of

B a C l_{2} (s)

is:

– 29.4 kJ
+ 11.8 kJ
– 11.8 kJ
29.4 kJ

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Q. Bond dissociation enthalpies of

H_{2 (g)}, C l_{2} a n d H C l_{(g)}

are 104, 58 and 103 kcal respectively. The enthalpy of formation of HCl is

- 44 kcal
- 88 kcal
- 22 kcal
- 11 kcal

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Q. The enthalpy change in the reaction,

2 C O + O_{2} ⟶ 2 C O_{2}

is termed as:

Enthalpy of reaction
Enthalpy of combustion
Enthalpy of formation
Enthalpy of fusion

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Heat of reaction for $C_{6} H_{12} O_{6} (s) + 6 O_{2} \to 6 C O_{2} (g) + 6 H_{2} O (v)$ at constant pressure is $- 651 K c a l$ at $17^{\circ} C$ . What is the heat of reaction at constant volume at $17^{\circ} C$ ?

-654.48 Kcal
-655.48 Kcal
-653.48 Kcal
None of these

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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

$+ 144.0 k J m o l^{(- 1)}$
$- 74.8 k J m o l^{(- 1)}$
$- 144.0 k J m o l^{(- 1)}$
$+ 78.8 k J m o l^{(- 1)}$

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