Hydrogen gas (a potential future fuel) can be formed by the...

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: $$\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{CO}(g)+3 \mathrm{H}_{2}(g)$$ In a particular reaction, 25.5 $\mathrm{L}$ of methane gas (measured at a pressure of 732 torr and a temperature of $25^{\circ} \mathrm{C} )$ mixes with 22.8 $\mathrm{L}$ of water vapor (measured at a pressure of 702 torr and a temperature of $125^{\circ} \mathrm{C}$ ). The reaction produces 26.2 $\mathrm{L}$ of hydrogen gas at STP. What is the percent yield of the reaction?

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation:
$$\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{CO}(g)+3 \mathrm{H}_{2}(g)$$
In a particular reaction, 25.5 $\mathrm{L}$ of methane gas (measured at a pressure of 732 torr and a temperature of $25^{\circ} \mathrm{C} )$ mixes with 22.8 $\mathrm{L}$ of water vapor (measured at a pressure of 702 torr and a temperature of $125^{\circ} \mathrm{C}$ ). The reaction produces 26.2 $\mathrm{L}$ of hydrogen gas at STP. What is the percent yield of the reaction?

Key Concepts

Reaction Stoichiometry

This concept involves the quantitative relationships between reactants and products in a chemical reaction based on a balanced equation. It is essential for determining the amount of product that can theoretically be obtained from given amounts of starting materials, as well as for identifying the limiting reactant.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Understanding and identifying the limiting reactant is key to calculating the theoretical yield and subsequently, the percent yield of a reaction.

Ideal Gas Law

The ideal gas law, represented by the equation PV = nRT, relates the pressure, volume, temperature, and number of moles of a gas. This principle is critical when dealing with gaseous reactants and products, especially when their conditions (such as pressure and temperature) differ from standard conditions.

Standard Temperature and Pressure (STP)

STP is a reference point commonly used in chemistry that denotes 0°C (273.15 K) and 1 atmosphere pressure. It allows for the standardization of gas volumes, meaning that gas volumes measured at different conditions can be converted to STP conditions for comparative purposes.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield derived from stoichiometry. This concept is important in both laboratory and industrial applications to assess the success of a reaction and the practical viability of a process.

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