Question

Using the information in the table, the rate law for the reaction A(g) + 3 B(g) ? C(g) + 2 D(g) is [A]? (M) | [B]? (M) | Rate (M/s) 1.25 | 0.100 | 0.850 1.25 | 0.300 | 2.55 3.75 | 0.200 | 5.10 A) Rate = k[A][B]3 B) Rate = k[B] C) Rate = k[A][B] D) Rate = k[A][B]2

          Using the information in the table, the rate law for the reaction A(g) + 3 B(g) ? C(g) + 2 D(g) is

[A]? (M) | [B]? (M) | Rate (M/s)
1.25 | 0.100 | 0.850
1.25 | 0.300 | 2.55
3.75 | 0.200 | 5.10

A) Rate = k[A][B]3
B) Rate = k[B]
C) Rate = k[A][B]
D) Rate = k[A][B]2

Using the information in the table, the rate law for the reaction A(g) + 3 B(g) ? C(g) + 2 D(g) is

[A]? (M) | [B]? (M) | Rate (M/s)
1.25 | 0.100 | 0.850
1.25 | 0.300 | 2.55
3.75 | 0.200 | 5.10

A) Rate = k[A][B]3
B) Rate = k[B]
C) Rate = k[A][B]
D) Rate = k[A][B]2

Added by Courtney M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

03/28/2023

Step 1

Let's label the rows of the table as experiments 1, 2, and 3. Experiment 1: Rate = 1.25 M/s [A] = 0.100 M [B] = 0.850 M Experiment 2: Rate = 1.25 M/s [A] = 0.300 M [B] = 0.850 M Experiment 3: Rate = 3.75 M/s [A] = 0.100 M [B] = 0.200 M Now, let's compare Show more…

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Using the information in the table, the rate law for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is [A]₀ (M) | [B]₀ (M) | Rate (M/s) 1.25 | 0.100 | 0.850 1.25 | 0.300 | 2.55 3.75 | 0.200 | 5.10 A) Rate = k[A][B]3 B) Rate = k[B] C) Rate = k[A][B] D) Rate = k[A][B]2