Question

Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(9) C(g) + 2 D(9) is [A]. (M) [B]. (M) Rate (M/min) A) 13.4 M™ min B) 0.13 min 0.300 0.180 0.0234 C) 0.259 min 0.300 0.360 0.0934 D) 0.26 M"min" E) 0.722 M" min 0.150 0.180 0.0234

Answer 1

By analyzing the data, it is clear that if we double the concentration of A keeping congratulation of B constant, rate remains same. It means order of reaction with respect to A is zero.

And if we double the concentration of B keeping concentration of A constant, rate of reaction becomes 4 times. It means order of reaction with respect to B is two.

rate lane can be written as: Rate =k [B] ² 0, 0234= K (0:18) K = 0.0234 0:18X0,18 = = 0.722 K=0.722 mal minrl