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Consider the following reaction in a closed reaction flask. If 1.00 atm of gas A is allowed to react with 1.00 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the reaction flask at the end of the reaction? What are the partial pressures of the gases in the flask?

6A(g) + 2B(g) ? 2A3B(g)

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Beverley Smith
Beverley SmithLv2
28 Sep 2019

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Related questions

Consider the following reaction in a closed reaction flask. If 1.50atm of gas A is allowed to react with 0.500 atm of gas B and thereaction goes to completion at constant temperature and volume,what is the total pressure in the reaction flask at the end of thereaction? What are the partial pressures of the gases in theflask?

4A(g) + 6B(g) ? 2A2B3(g)

A. (0.750 atm A2B3 produced) + (0.25 atm B remaining) = 1.00 atmtotal pressure
B. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atmtotal pressure
C. (1.50 atm A2B3 produced) + (0.167 atm A remaining) = 1.67 atmtotal pressure
D. (0.333 atm A2B3 produced) + (0.500 atm A remaining) = 0.833 atmtotal pressure

Consider the following reaction : 2A(g) + B2(g) ? 2AB(g)

If 1.20 atm of A is mixed with 2.00 atm of B2 in a closed constant-volume reaction flask, what would be the final pressure in the reaction flask at the end of the reaction (assume the reaction goes to completion and that the temperature does not change) ?

When a 2.00 L flask containing 1.50 atm of gas A is joined with a 2.50 L flask containing 0.350 atm of gas B, and the stopcock between the flasks is opened, and the gases are allowed to mix thoroughly, the following reaction proceeds at constant temperature. What is the resulting total pressure of gases in now-joined flasks after the reaction proceeds to completion?????????? help

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