C
1) Use the experimental data to determine the rate constant for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.20 |
0.20 |
0.144 |
2 |
0.40 |
0.20 |
0.288 |
3 |
0.20 |
0.40 |
0.576 |
Rate = k[A][B]2
(a) 18 L2/mol2·s
(b) 0.06 L2/mol2·s
(c) 3.6 L2/mol2·s
(d) 18 L/mol·s
2) Use the experimental data to determine the rate equation for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.20 |
0.20 |
0.145 |
2 |
0.20 |
0.60 |
0.435 |
3 |
0.60 |
0.20 |
1.305 |
(a) Rate = k[A][B]
(b) Rate = k[A]2[B]2
(c) Rate = k[A]2[B]
(d) Rate = k[A][B]2
3) Use the experimental data to determine the rate equation for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.20 |
0.20 |
0.150 |
2 |
0.20 |
0.60 |
0.150 |
3 |
0.60 |
0.20 |
1.350 |
(a) Rate = k[A][B]2
(b) Rate = k[A]2[B]2
(c) Rate = k[A]2[B]
(d) Rate = k[A]2
4) Use the experimental data to determine the rate constant for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.20 |
0.20 |
0.156 |
2 |
0.40 |
0.20 |
0.312 |
3 |
0.20 |
0.40 |
0.312 |
Rate = k[A][B]
(a) 0.26 L/mol·s
(b) 3.9 L/mol·s
(c) 3.9 L2/mol2·s
(d) 0.26 L2/mol2·s
5) Use the experimental data to determine the rate equation for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.30 |
0.30 |
0.170 |
2 |
0.90 |
0.30 |
0.170 |
3 |
0.30 |
0.90 |
1.530 |
(a) Rate = k[A][B]
(b) Rate = k[A]2[B]
(c) Rate = k[B]2
(d) Rate = k[A][B]2
6) Use the experimental data to determine the rate constant for the following reaction.
3A + B
C
Trial |
[A] |
[B] |
Initial Rate |
1 |
0.30 |
0.30 |
0.170 |
2 |
0.90 |
0.30 |
0.170 |
3 |
0.30 |
0.90 |
1.530 |
Rate = k[B]2
(a) 0.53 L/mol·s
(b) 1.9 s-1
(c) 1.9 L/mol·s
(d) 0.53 s-1