A certain substance, initially present at 0.950 M, decomposes by first-order kinetics with a rate constant of 1.25 × 102 mol L 's'!. Calculate the time (in seconds) required for the system to reach a concentration of 0.555M. seconds Submit Hide Hints Hint 1 Hint 2 The integrated rate law for this reaction is (A)- kt + (Alo OMA) - k+ MA O la[A] -kt + In[A]o OMA)- kt+ MA

At a certain temperature the rate of this reaction is first order in SO; with a rate constant of 0.00824 s: 2so; (2) - 2 So, (2) +0, (g) Suppose a vessel contains SO, at a concentration of 1.01 M. Calculate the concentration of So; in the vessel 73.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

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Correct Expressed in terms of x, y, and z, the rate law is as follows: The iodate ion, IO3¯, is reduced by sulfite, SO32", according to the following net ionic equation: rate = kæyz By substituting the actual species from the reaction, the expression becomes I03 (aq) + 3S03²- (aq)→I¯(aq) + 3SO,²-(aq) k[IO3 ][SO3²-][H*] rate = Part B By what factor will the rate of the reaction change if the pH changes from 6.50 to 2.00? Express your answer numerically using two significant figures. • View Available Hint(s) 3.2 • 10-5 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Because it is less than one, your answer implies that the rate decreases. However, lowering the pH raises the hydrogen ion concentration. Part C The reaction is pH dependent even though the H+ ion does not appear in the overall reaction. Which of the following explains this observation? Check all that apply. • View Available Hint(s) O H+ serves as a catalyst in the reaction. The exponent of H+ in the rate…