Question

The value of $ {{K}_{p}} $ for the reaction, $ 2{{H}_{2}}S(g)2{{H}_{2}}(g)+{{S}_{2}}(g) $ is $ 1.2\times {{10}^{-2}} $ $ {{1065}^{o}}C. $ The value for $ {{K}_{c}} $ is

• A. $ <1.2\times {{10}^{-2}} $
• B. $ >1.2\times {{10}^{-2}} $
• C. $ 1.2\times {{10}^{-2}} $
• D. $ 0.12\times {{10}^{-2}} $

Answer 1

Answer: (A)

$ \Delta {{n}_{g}}= $ moles of gaseous products - moles of gaseous reactants, = 3 ? 2 ? 1 = 0 $ {{K}_{p}}={{K}_{c}}{{(RT)}^{\Delta {{n}_{g}}}} $ $ {{K}_{c}}=\frac{{{K}_{p}}}{RT} $ $ =\frac{1.2\times {{10}^{-2}}}{0.0821\times 1338} $ $ =1.09\times {{10}^{-4}}<1.2\times {{10}^{-2}} $