For the gaseous reaction involving the complete combustion of isobutane:

△ H = △ E

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△ H > △ E

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△ H = △ E = 0

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△ H < △ E

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Solution

The correct option is B $△ H > △ E$
Enthalpy of reaction is given by,

$Δ H = Δ E + n_{g} R T$

Combustion of isobutane-

$C_{4} H_{1} 0 + \frac{13}{2} O_{2} ⟶ 4 C O_{2} + 5 H_{2} O$

As the $Δ n_{g} > 0$

$∴ Δ H > Δ E$

Hence, option $B$ is correct.

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Similar questions

Q. For the gaseous reaction involving complete combustion of isobutane (assuming all products and reactants are in gaseous state), the relation between

Δ H

and

Δ E

will be:

Q. For the half cell reaction at 298 K,

H^{+} (a q) + e^{-} \to \frac{1}{2} H_{2} (g) (1 atm)

Q. For the combustion of

C_{6} H_{10}

with the required amount of oxygen, which of the following is correct? (Where reactants and products are in their standard states)

$E_{0}$ and $E_{h}$ respectively represent the average kinetic energy of a molecule of oxygen and hydrogen. If the two gases are at the same temperature, which of the following statements is true?

Δ H < Δ E

for the reaction:

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For the gaseous reaction involving the complete combustion of isobutane:

The correct option is B △H>△EEnthalpy of reaction is given by,ΔH=ΔE+ngRTCombustion of isobutane-C4H10+132O2⟶4CO2+5H2OAs the Δng>0∴ΔH>ΔEHence, option B is correct.

The correct option is B $△ H > △ E$
Enthalpy of reaction is given by,

$Δ H = Δ E + n_{g} R T$

Combustion of isobutane-

$C_{4} H_{1} 0 + \frac{13}{2} O_{2} ⟶ 4 C O_{2} + 5 H_{2} O$

As the $Δ n_{g} > 0$

$∴ Δ H > Δ E$

Hence, option $B$ is correct.