Part A) The rate constant for a certain reaction is k = 8.80×10−3 s−1. If the initial reactant concentration was 0.550 M, what will the concentration be after 18.0 minutes? Express your answer with the appropriate units.   Part B)   A zero-order reaction has a constant rate of 3.80×10−4 M/s. If after 45.0 seconds the concentration has dropped to 4.50×10−2 M, what was the initial concentration? Express your answer with the appropriate units.

Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.

Consider the hypothetical reaction: A + B + 2C → 2D + E where the rate law is Rate = -ALA) = k[A][B]2 An experiment is carried out where [Alo = 7.200 x 102 M, [B]. = 2.500 M and [Cla = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M2s1. Answer:

The following chemical reaction: A → products shows second order kinetics with respect to A; rate = K[A]². If k = 11.99 x 10-³ mol-¹ L s¯¹ and the initial concentration of A is 1.45 mol L-1, what is the half life of this reaction in minutes? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:

The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.

NOBr(g) decomposes to form NO and Br2 by the reaction 2 NOBr(g) + 2 NO(g) + Br2(8) It is found that the reaction is second order in NOBr. The rate constant has been found to be 0.170 M-1 s1. In a situation where the initial concentration of NOBr in a vessel is 0.690 M, how long will it take for the concentration of Br2 to reach 0.180 M? (Assume, of course, that there was no Br in the vessel to begin with.) Report your result in seconds with one decimal place but do not put units in the

After 48 seconds, 10.% of reactant has reacted. If the reaction is a 1st order reaction, the special rate constant k = _.

The decomposition of ethylene oxide (CH₂)2O(g) → CH4(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 631 K.

The thermal decomposition of phosphine into phosphorus and hydrogen is a first order reaction with a half-life of 35.0 s at 680 °C.  4 PH3 (g) → P4 (g) + 6 H2 (g)  a) Write the rate law for this reaction. b) How much time (in minutes) is required for 97% of a phosphine sample to decompose at 680 °C?  c) If the activation barrier is 3.05 x 105 J/mol, what is the half-life for this reaction at 710 °C?

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