When solid mercury(I) carbonate, Hg2CO3, is added to nitric acid, HNO3, a reaction occurs to give mercury(II) nitrate, Hg1NO322, water, and two gases A and B: Hg2CO31s2 + HNO31aq2¡ Hg1NO3221aq2 + H2O1l 2 + A1g2 + B1g2 (a) When the gases are placed in a 500.0-mL bulb at 20 °C, the pressure is 258 mm Hg. How many moles of gas are present?

검증된 단계별 안내

Identify the gases A and B produced in the reaction. In this reaction, the gases are likely carbon dioxide (CO2) and nitrogen dioxide (NO2).

Use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.

Convert the given pressure from mm Hg to atmospheres (atm) as the gas constant R is typically used with pressure in atm. Use the conversion factor 1 atm = 760 mm Hg.

Convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Substitute the converted pressure, the volume in liters, the converted temperature, and the gas constant (use R = 0.0821 L atm / K mol for consistency) into the ideal gas law equation to solve for n, the number of moles of gas.

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영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. Here, P is the pressure in atmospheres, V is the volume in liters, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. This law is essential for calculating the number of moles of gas produced in a reaction when given the pressure, volume, and temperature.

Gas Pressure Units

Gas pressure can be measured in various units, including mm Hg, atm, and pascals. In this question, the pressure is given in mm Hg, which can be converted to atmospheres (1 atm = 760 mm Hg) for use in the Ideal Gas Law. Understanding how to convert between these units is crucial for accurate calculations in gas-related problems.

Stoichiometry of Gas Reactions

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In this case, knowing the balanced chemical equation allows us to determine the moles of gases produced from the reaction of mercury(I) carbonate with nitric acid. This understanding is vital for calculating the number of moles of gases A and B formed during the reaction.