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The decomposition of NH_(3) on platinum surface, 2 NH_(3)(g)overset(Pt)toN_(2)(g)+3H_(2)(g),is zero order with k=2*5xx10^(-4)molL^(-1)s^(-1). What are the rates of production of N_(2) and H_(2) ? |
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Answer» Solution :`2 NH_(3)toN_(2)+3 H_(2)," Rate"=-(1)/(2)(d[NH_(3)])/(dt)=+(d[N_(2)])/(dt)=+(1)/(3)(d[H_(2)])/(dt)` For zero ORDER reaction, rate `=k:.-(1)/(2)(d[NH_(3)])/(dt)=(d[N_(2)])/(dt)=(1)/(3)(d[H_(2)])/(dt)=2*5xx10^(-4)molL^(-1)s^(-1)` `:." Rate of PRODUCTION of "N_(2)=(d[N_(2)])/(dt)=2*5xx10^(-4)molL^(-1)s^(-1)` Rate of production of `H_(2)=(d[H_(2)])/(dt)=3xx(2*5xx10^(-4)molL^(-1)s^(-1))=7*5xx10^(-4)molL^(-1)s^(-1)`. |
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