Consider the following reaction: 2HBr(g) rightarrow H2(g) + Br2(g) Express the r

Question

Consider the following reaction: 2HBr(g) rightarrow H2(g) + Br2(g) Express the rate of the reaction with respect to each of the reactants and products. Rate = 1 / 2 Delta[HBr] / Delta t = Delta[H2] / Delta t = Delta [Br2] / Delta t Rate = Delta [HBr] / Delta t = 1 / 2 Delta [H2] / Delta t = -1 / 2 Delta [Br2] / Delta t Rate = -1 / 2 Delta [HBr] / Delta t = Delta [H2] / Delta t = Delta [Br2] / Delta t Rate = Delta [HBr] / Delta t = 1 / 2 Delta [H2] / Delta t = 1 / 2 Delta [Br2] / Delta t In the first 18.0s of this reaction, the concentration of HBr dropped from 0.510M to 0.450M. Calculate the average rate of the reaction in this time interval. Express your answer using two significant figures. If the volume of the reaction vessel in part (b) was 0.500 L, what amount of Br2 (in moles) was formed during the first 18.0s of the reaction? Express your answer using two significant figures.

Explanation / Answer

B) 1.6667*10^-3 C) 0.015 moles

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