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1 mole of NO2 and 2 moles of CO are enclosed in a one litre vessel to attain the following equilibrium 
NO2​+CO ⇌ NO+CO2​ I twas estimated that at the equilibrium, 25% of initial amount of CO is consumed. The equilibrium constant Kp​ is 

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\\\text{According to question.........} \\ \text{since 1 mole of } \mathrm{N} \mathrm{O}_{2} \text{ reacts with 1 mole of } \mathrm{CO}, \\ \text{ thus 25 percent of CO is 1 / 2 moles out of 2 moles have reacted with 1 / 2 moles of } \mathrm{N} \mathrm{O}_{2}.

\begin{array}{l} \mathrm{Kc}=\frac{1}{2} \times \frac{1}{2}=\frac{1}{4} \times \frac{4}{3}=\frac{1}{3} \\ \mathrm{Kp}=\mathrm{Kc}(\mathrm{RT}) \Delta \mathrm{n} \end{array}

\\\Delta \mathrm{n}=\text{ change in no. of moles } = \text{ no. of mole of product - no. of moles of reactant. } \\ \Delta \mathbf{n}=(1+1)-(1+1)=0 \\ \text{thus,} \\ \therefore \quad \mathrm{Kp}=\mathrm{Kc}=1 / 3

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