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For the first order thermal decomposition reaction, the following data were obtained: C_(2)H_(5)Cl(g) to C_(2)H_(4)(g)+HCl(g) {:("Time/second","Total pressure/atm"),(""0,""0.30),(""300,""0.50):} Calculate the rate constant. [Given : log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021] |
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Answer» Solution :Apply the relation for first order REACTION for gaseous state `K=(2.303)/(t)"LOG"(p_(i))/(2p_(i)-p_(t))` Substituting the values, we have `k=(2.303)/(300)"log"(0.3)/(0.6-0.5)=(2.303)/(300)log3=(2.303)/(300s)xx0.4771=0.0037s^(-1)` |
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