164036 Two moles of gas \(A_2\) are mixed with two moles of gas \(B_2\) in a flask of volume 1 litre. If at equilibrium 0.5 moles of \(A_2\) are obtained. Then find out \(K_P\) for reaction \(\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})\)

164037 For the reaction \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\), the equilibrium constant is \(K_1\). The equilibrium constant is \(K_2\) for the reaction
\(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g}) \text {. }\)
What is \(K\) for the reaction
\( \mathrm{NO}_2(\mathrm{~g}) \rightleftharpoons 1 / 2 \mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \)

164038 The \(K_a\) for a weak acid \(H X\) is \(10^{-6}\), then the ionisation constant of \(\mathrm{X}^{-}\)will be:

164039 Find out the value of \(\alpha\) of \(10^{-2} \mathrm{M} \mathrm{NH}_4 \mathrm{OH}\) solution if \([\mathrm{OH}]=10^{-3}\)

164036 Two moles of gas \(A_2\) are mixed with two moles of gas \(B_2\) in a flask of volume 1 litre. If at equilibrium 0.5 moles of \(A_2\) are obtained. Then find out \(K_P\) for reaction \(\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})\)

164037 For the reaction \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\), the equilibrium constant is \(K_1\). The equilibrium constant is \(K_2\) for the reaction
\(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g}) \text {. }\)
What is \(K\) for the reaction
\( \mathrm{NO}_2(\mathrm{~g}) \rightleftharpoons 1 / 2 \mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \)

164038 The \(K_a\) for a weak acid \(H X\) is \(10^{-6}\), then the ionisation constant of \(\mathrm{X}^{-}\)will be:

164039 Find out the value of \(\alpha\) of \(10^{-2} \mathrm{M} \mathrm{NH}_4 \mathrm{OH}\) solution if \([\mathrm{OH}]=10^{-3}\)

164036 Two moles of gas \(A_2\) are mixed with two moles of gas \(B_2\) in a flask of volume 1 litre. If at equilibrium 0.5 moles of \(A_2\) are obtained. Then find out \(K_P\) for reaction \(\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})\)

164037 For the reaction \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\), the equilibrium constant is \(K_1\). The equilibrium constant is \(K_2\) for the reaction
\(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g}) \text {. }\)
What is \(K\) for the reaction
\( \mathrm{NO}_2(\mathrm{~g}) \rightleftharpoons 1 / 2 \mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \)

164038 The \(K_a\) for a weak acid \(H X\) is \(10^{-6}\), then the ionisation constant of \(\mathrm{X}^{-}\)will be:

164039 Find out the value of \(\alpha\) of \(10^{-2} \mathrm{M} \mathrm{NH}_4 \mathrm{OH}\) solution if \([\mathrm{OH}]=10^{-3}\)

164036 Two moles of gas \(A_2\) are mixed with two moles of gas \(B_2\) in a flask of volume 1 litre. If at equilibrium 0.5 moles of \(A_2\) are obtained. Then find out \(K_P\) for reaction \(\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})\)

164037 For the reaction \(\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})\), the equilibrium constant is \(K_1\). The equilibrium constant is \(K_2\) for the reaction
\(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g}) \text {. }\)
What is \(K\) for the reaction
\( \mathrm{NO}_2(\mathrm{~g}) \rightleftharpoons 1 / 2 \mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \)

164038 The \(K_a\) for a weak acid \(H X\) is \(10^{-6}\), then the ionisation constant of \(\mathrm{X}^{-}\)will be:

164039 Find out the value of \(\alpha\) of \(10^{-2} \mathrm{M} \mathrm{NH}_4 \mathrm{OH}\) solution if \([\mathrm{OH}]=10^{-3}\)