+ 100% 4) The rate law for the decomposition of N20s is Rate kIN20s], where k 5.

Question

+ 100% 4) The rate law for the decomposition of N20s is Rate kIN20s], where k 5.0 x 10' s What is the concentration of N205 after 1900 s, if the initial concentration is 0.56 M? 5.) The reaction 2N0(g) + 2H2(g) N2 (g) + 2 H2O (g) has been studied at 904°C. Ex. No. Initial [NO] Initial [H2l Initial Rate of formation of N2 (M sec) 0.420 M 0.210 M 0.210 M 0.105 M 0.136 00339 0.0678 0.0339 0.122 M 0.122 0.244 M 4 0.488 M a.) Write the rate equation for the reaction. b.) Calculate the rate constant at 904°C. c.) Find rate of appearance of N2 at the instant when [NO] = 0.550 M and [H2-199 M 6) The reaction 2NO(g) + 2 H2(g) N2(g) + 2 H2O(g) is found experimentally to be second order in NO(g) and first-order in H2(g). (a) Write the rate law for the reaction. (b) What is the overall order of the reaction? (c) What are the units for the rate constant k? (d) If INOJ is doubled (while keeping [H2l constant), by what factor will the reaction rate increase? (e) If [H2] is doubled (while keeping [NO] constant), by what factor will the reaction rate increase?

Explanation / Answer

4) This is a first order chemical kinetics reaction .

kt = 2.303 log(initial conc./final conc.)

5 X 10-4 X 1900 = 2.303 log( 0.56/x)

So we have to find x that is the final concentration after 1900s

Final concentration = 0.2166 M

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