Question

A rigid stainless steel chamber contains 260 Torr of methane, CH4, and excess oxygen, O2, at...

A rigid stainless steel chamber contains 260 Torr of methane, CH4, and excess oxygen, O2, at 170.0 °C. A spark is ignited inside the chamber, completely combusting the methane. What is the change in total pressure within the chamber following the reaction? Assume a constant temperature throughout the process.

ΔP = _________ Torr

Homework Answers

Answer #1

CH4 + 2O2 ---> CO2 + 2H2O

According the above reaction

260 torr of CH4 pressure means at least 520 torr of O2 pressure. Since it is excess, let us call the O2 pressure 520 + x.
Let us consider the CH4 to CO2 molar ratio of 1 to 1. Since this happens at constant volume and constant temperature, the pressures are directly related to the moles used and produced. Thus, we conclude 260 torr of CO2 pressure is produced.
Since we are at 170 C, the water produced is gaseous. Let us consider the CH4 to H2O molar ratio of 1 to 2. This informs us that 520 torr of water vapor pressure is created.
Since O2 is in excess, we know that x remains after 520 torr of O2 is used up. I know 520 torr of O2 is used because of the CH4 to O2 molar ratio in the balanced equation.

Conclusion: no pressure change in the chamber at reaction's end.

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