Standard Temperature and Pressure Video Lessons

Concept: Understanding Standard State Conditions

# Problem: Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4(g) + H2O(g) → CO(g) + 3 H2(g)In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

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Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation:

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

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Based on our data, we think this problem is relevant for Professor Bruehl's class at CU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: A Molecular Approach - Tro 2nd Edition. You can also practice Chemistry: A Molecular Approach - Tro 2nd Edition practice problems.