Gas A decomposes at 600 K into two gases B and C and the decomposition is catalyzed by gas B as shown below: A(g)+B(g)→C(g)+3B(g) The rate law is r = k[A][B]. If initially in a one-liter container, 5 mol A, 2 mol B are taken at 600 K, and the reaction starts with an initial rate of 4.0 molL−1s−1 then, what will be the maximum rate (in Mol/Ls) of the reaction that it can have during the whole reaction time?

Gas A decomposes at 600 K into two gases B and C and the decomposition

1.	Gas A decomposes at 600 K into two gases B and C and the decomposition is catalyzed by gas B as shown below: A(g)+B(g)→C(g)+3B(g) The rate law is r = k[A][B]. If initially in a one-liter container, 5 mol A, 2 mol B are taken at 600 K, and the reaction starts with an initial rate of 4.0 molL−1s−1 then, what will be the maximum rate (in Mol/Ls) of the reaction that it can have during the whole reaction time?
Answer» Gas A decomposes at 600 K into two gases B and C and the decomposition is catalyzed by gas B as shown below: $A_{(g)} + B_{(g)} \to C_{(g)} + 3 B_{(g)}$ The rate law is r = k[A][B]. If initially in a one-liter container, 5 mol A, 2 mol B are taken at 600 K, and the reaction starts with an initial rate of $4.0 m o l L^{- 1} s^{- 1}$ then, what will be the maximum rate (in Mol/Ls) of the reaction that it can have during the whole reaction time?