At 300°C decomposition of NO₂(g)occurs with a rate law: Rate = - k[NO₂]^x.If the initial rate of decomposition is 3.2 × 10^-5M/s when [NO₂]_o = 8.0 × 10^-3 M and the initial rate of decomposition is 8.0 × 10^-6M/s when [NO₂]_o = 4.0 × 10^-3 M,then the order of reaction with respect to NO₂,x = ________.

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The Answer of At 300°C decomposition of NO₂(g)occurs with a rate law: Rate = - k[NO₂]^x.If the initial rate of decomposition is 3.2 × 10^-5M/s when [NO₂]_o = 8.0 × 10^-3 M and the initial rate of decomposition is 8.0 × 10^-6M/s when [NO₂]_o = 4.0 × 10^-3 M,then the order of reaction with respect to NO₂,x = ________.

At 300°C Decomposition of NO2(g)occurs with a Rate Law: Rate

At 300°C Decomposition of NO₂(g)occurs with a Rate Law: Rate