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A gas mixture at 0°C and 1.0 atm contains 0.010 mol of H₂, 0.015 mol of O₂, and 0.025 mol of N₂. Assuming ideal behavior, what is the partial
A gas mixture at 0°C and 1.0 atm contains 0.010 mol of H₂, 0.015 mol of O₂, and 0.025 mol of N₂. Assuming ideal behavior, what is the partialpressure of hydrogen gas (H₂) in the mixture?
Final answer:The partial pressure of hydrogen gas (H₂) in the gas mixture is 0.200 atm.Explanation:The partial pressure of hydrogen gas (H₂) in the gas mixture can be determined using Dalton's law of partial pressures. According to this law, the total pressure of the mixture is the sum of the partial pressures of each gas component. In this case, we have0.010 molof H₂, which means the partial pressure of H₂ can be calculated as follows:Calculate the moles of H₂:0.010 mol of H₂Calculate the mole fraction of H₂:H₂ mole fraction = (moles of H₂) / (total moles of all gases)H₂ mole fraction = 0.010 / (0.010 + 0.015 + 0.025)Calculate the partial pressure of H₂:H₂ partial pressure = H₂ mole fraction * total pressure of the mixtureH₂ partial pressure = (0.010 / 0.050) * 1.0 atmTherefore, the partial pressure of hydrogen gas (H₂) in the mixture is0.200 atm.Learn more about Partial pressure of hydrogen gas in a mixture here:brainly.com/question/9148379...