Question

Answering all three questions would really help

What is the rate at which Br(aq) disappears in the reaction below if the rate of disappearance of BrO3-(aq) is 0.045 M/s? BrO3 + 5 Br + 6 H+ + 3 Br2 + 3H2O M/s How long will it take for the concentration of A to decrease from 0.500 M to 0.130 M in the first-order reaction A →B? (k = 0.800 s-1) S The reaction A+B 2 C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when [A] remains constant but [B] is doubled?

Answer 1

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1 Broz + 5 Br- + 6Ht 3Br . t 3tho d[Bro 3] -dBv] 5 di - d[Br] dr - d[er] 025 Mls. di => 0.045M/s x 5 This the rate of disappearance of Br is 0.225 M/s. - ln 0.5 0:13 we have kt - ln [Alo TA) t- 0.85 t = 1.685 rate = K[A] [B]} T ( [B] is doubled than when 8k [n] [B] rate - Km 20873 8 The rate increases