Determine the rate law and the value of k for the following reaction using the d

Question

Determine the rate law and the value of k for the following reaction using the data provided. S2O8 2 -(aq) + 3 I-(aq) ? 2 SO4 2 -(g) + I3 -(aq) [S2O8 2 -]i (M) [I-]i (M) Initial Rate (M-1s-1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 Determine the rate law and the value of k for the following reaction using the data provided. S2O8 2 -(aq) + 3 I-(aq) ? 2 SO4 2 -(g) + I3 -(aq) [S2O8 2 -]i (M) [I-]i (M) Initial Rate (M-1s-1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 Rate = 195 M-3s-1 [S2O8 2 -]2[I-]2 Rate = 36 M-1s-1 [S2O8 2 -][I-] Rate = 23 M-1/2s-1 [S2O8 2 -][I-]1/2 Rate = 120 M-2s-1 [S2O8 2 -]2[I-] Rate = 86 M-2s-1 [S2O8 2 -][I-]2

Explanation / Answer

Soe the rate law would be rate = k[A][B]. So then you plug in one of the experiments and solve for k(the rate constant.) If you use experiment one: 2.2 x 10^-4 = k (.080) (.034) k = .08088 k = 8.09 x 10^-2 I believe this is right, you might want to double check my math because i used my computer's calculater

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.