A chemist conducted a study of the decomposition of phosphine gas, PH3 (g), into phosphorous gas, P4(g), and hydrogen gas. This reaction is represented by the following balanced chemical equation: 4 PH3(g) → P4(g) + 6 H2(g) She determined the rate of reaction with respect to the consumption of phosphine gas to be -0.0024 mol/(L s). What are the rates of formation of phosphorous gas and hydrogen gas in this experiment? Place your answer for phosphorous gas in the first blank and your answer for hydrogen gas in the second blank.

A chemist conducted a study of the decomposition of phosphine gas, PH3 (g), into phosphorous gas, P4(g), and hydrogen gas. This reaction is represented by the following balanced chemical equation: 4 PH3(g) → P4(g) + 6 H2(g) She determined the rate of reaction with respect to the consumption of phosphine gas to be -0.0024 mol/(L s). What are the rates of formation of phosphorous gas and hydrogen gas in this experiment? Place your answer for phosphorous gas in the first blank and your answer for hydrogen gas in the second blank.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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