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Ideal Gas Equation

The dissociat...

Question

The dissociation of $C O_{2}$ can be expressed as $2 C O_{2} ⇌ 2 C O + O_{2}$ . If the 2 moles of $C O_{2}$ is taken initially and 40% of the $C O_{2}$ is dissociated equilibrium then total number of moles at equilibrium is:

2.4

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1.2

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Solution

The correct option is A 2.4
$2 C O_{2} ⇌ 2 C O$ $+$ $O_{2}$

Initial $2$ $0$ $0$
Final $2 - \frac{40}{100} \times 2$ $0.4 \times 2$ $0.4$
Total moles $= 2 - 0.4 \times 2 + 0.4 \times 2 + 0.4 = 2.4$

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Similar questions

Q. The dissociation of

C O_{2}

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2 C O_{2} ⇌ 2 C O + O_{2}

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40 %

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Q. If the equilibrium constant for reaction (i) is 2, what is the equilibrium constant for reaction (ii)?

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.... (ii)

At 3000 K the equilibrium pressures of $C O_{2},$ CO and $O_{2}$ are 0.6, 0.4 and 0.2 atmospheres respectively. $K_{p}$ for the reaction, $2 C O_{2} ⇌ 2 C O + O_{2}$ is

Q. The degree of dissociation of

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α

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Q. If, in the reaction

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Initial	$2$	$0$	$0$
Final	$2 - \frac{40}{100} \times 2$	$0.4 \times 2$	$0.4$

The dissociation of CO2 can be expressed as 2CO2⇌2CO+O2. If the 2 moles of CO2 is taken initially and 40% of the CO2 is dissociated equilibrium then total number of moles at equilibrium is:

The correct option is A 2.4 2CO2⇌2CO + O2 Initial 2 00 Final 2−40100×2 0.4×2 0.4Total moles=2−0.4×2+0.4×2+0.4=2.4

The dissociation of $C O_{2}$ can be expressed as $2 C O_{2} ⇌ 2 C O + O_{2}$ . If the 2 moles of $C O_{2}$ is taken initially and 40% of the $C O_{2}$ is dissociated equilibrium then total number of moles at equilibrium is:

The correct option is A 2.4
$2 C O_{2} ⇌ 2 C O$ $+$ $O_{2}$

Initial $2$ $0$ $0$
Final $2 - \frac{40}{100} \times 2$ $0.4 \times 2$ $0.4$
Total moles $= 2 - 0.4 \times 2 + 0.4 \times 2 + 0.4 = 2.4$