Calorific value of ethane- in kJ-g if for the reaction - 2C2H6 - 7O2 - 4CO2 - 6H2O- - H - -745-6 kcal

The correct option is B 52 2C_2H_6+7O_2→ 4CO_2+6H_2O ; Δ H= 745.6KCal ∴ Heat of combustion of ethane = 745.62= 372.8 Kcal #160; ...

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Standard XII

Chemistry

Types of Equillibrium

Calorific val...

Question

Calorific value of ethane, in kJ/g if for the reaction :

$2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O; Δ H = - 745.6 k c a l$

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Solution

The correct option is B $- 52$
$2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O$ ; $Δ H = - 745.6 K C a l$

$∴$ Heat of combustion of ethane $= \frac{- 745.6}{2} = - 372.8 K c a l$
$= - 372.8 \times 4.18 k J$

$= - 1558.3 k J$

Calorific value $= \frac{Heat of combustion}{Molecular weight of C_{2} H_{6}} = - \frac{1558.3}{30} = - 51.9 = - 52 k J / g$ .

Therefore, the correct option is B.

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Similar questions

Q. Calorific value of ethane, in kJ/g if for the reaction is:

2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O; Δ H = - 745.6

kcal.

Q. Calorific value of ethane, in KJ/g for the reaction

2 C_{2} H_{6} + 7 O_{7} ⟶ 4 {C O}_{2} + 6 H_{2} O

;

Δ H = - 745.6 K c a l

What volume of oxygen would be required for complete combustion of 100 litres of ethane according to the following equation?
2C₂H₆ + 7O₂ $\overset{}{\to}$ 4CO₂ + 6H₂O

Q. What volume of oxygen would be required for the complete combustion of 100 litres of ethane according to the following equation?

2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O

Q. Ethane burns in oxygen to form

C O_{2}

and

H_{2} O

according to the equation:

2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O

.
If

1250

cc of oxygen is burnt with

300

cc of ethane.
Calculate:
(i) the volume of

C O_{2}

formed.
(ii) the volume of unused

O_{2}

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Calorific value of ethane, in kJ/g if for the reaction : 2C2H6+7O2→4CO2+6H2O;ΔH=−745.6 kcal

The correct option is B −522C2H6+7O2→4CO2+6H2O; ΔH=−745.6KCal∴ Heat of combustion of ethane =−745.62=−372.8Kcal =−372.8×4.18kJ =−1558.3kJCalorific value =Heat of combustionMolecular weight of C2H6=−1558.330=−51.9=−52 kJ/g .Therefore, the correct option is B.

Calorific value of ethane, in kJ/g if for the reaction :

$2 C_{2} H_{6} + 7 O_{2} \to 4 C O_{2} + 6 H_{2} O; Δ H = - 745.6 k c a l$