Chem 2Exam #2February 27, 2004Key #11.The following reaction was observed for nitrous oxide (N2O):2 N2O(g)÷2 N2(g)+ O2(g)The concentration of N2was measured as a function of time. The rate of the reaction isequal to:a)b)c)rateNt= −∆∆2rateNt=∆∆2rateNt=22∆∆d)e)rateNt=∆∆22rateNt= −∆∆222.For the following reaction:2 N2O5(g)÷4 NO2(g)+ O2(g)the empirical rate law was:rate = k [N2O5]What are the units of k if the concentration of N2O5is measured in atm?3.Using the reaction and empirical rate law in Question #2, the initial rate for the reactionwas found to be 6.08 x 10-6atm/s when the initial pressure of N2O5was 0.010 atm. Whatwill be the rate when the pressure of N2O5is 0.0020 atm?
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4.For the following reaction:NO2(g)+ CO(g)6NO(g)+ CO2(g)the data below were obtained:[NO2], atm[CO], atmrate, atm/s2.00.506.0 x 10-32.80.501.2 x 10-22.01.56.0 x 10-3What is the order of the reaction with respect to NO2?5.Using the data and reaction in Question #4, what is the order of the reaction with respectto CO?a)zero orderb)first orderc)second orderd)half-ordere)third order6.For the following reaction:2 NO2(g)+ F2(g)÷2 NO2F(g)the empirical rate law was:rate = k [NO2] [F2]What is the value of k if the initial rate 4.9 x 10-3atm/s when the pressure of NO2is0.024 atm and the pressure of F2is 0.12 atm?