A particular first order reaction has a rate constant of 0.33 min^-1 How many mi

Question

A particular first order reaction has a rate constant of 0.33 min^-1 How many minutes will it take for a reactant concentration of 0.13 M to decrease to 0.088 M? 0.51 0.13 1.2 1.4 Consider the following equation PCl_5(g) doubleheadarrow PCl_3(g) + Cl_2(g) Initially, 0.84 mole of PCI_5 is placed in a 1.01. flask. At equilibrium. 0.72 mole of PCl_5 is present What is the value of K_c for this reaction? 0.72 0.12 0 0.62 0.020 The reaction below follows second-order kinetics and has a rate constant k, of 0.538 M^-1 sec^-1 use the integrated rate law to determine how long it will take for the concentration of NO_2 to drop from an initial value of 0.0100 M to 0.00650 M 2 NO_2 rightarrow 2 NO + O_2

Explanation / Answer

8) for first order reaction

K = (2.303 / t) log [A0] / [A]

0.33 = (2.303 /t) log [0.13] / [0.088]

0.33 = (2.303 / t) x 0.17

2.303 /t = 1.941

t = 1.12

answer = option c = 1..2 minutes

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