A mixture consisting of 0.140 mol N₂,0.037 mol O₂,0.104 mol CH₄,and an unknown amount of CO₂ occupies a volume of 8.48 L at 27°C and 1.06 atm pressure.How many moles of CO₂ are there in this sample? A)0.719 mol B)0.0839 mol C)2.45 mol D)3.77 mol E)0.364 mol

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Quizplus · Accepted Answer

First, we need to calculate the total amount of moles in the mixture: 0.140 mol N₂ + 0.037 mol O₂ + 0.104 mol CH₄ + x mol CO₂ = total amount of moles Simplifying: 0.281 + x = total amount of moles Next, we can use the ideal gas law to find the total number of moles: PV = nRT n = PV/RT = (1.06 atm)(8.48 L)/(0.0821 L·atm/(mol·K))(300 K) = 3.22 mol Substituting n into our equation: 0.281 + x = 3.22 x = 2.94 mol Therefore, there are 2.94 mol of CO₂ in the mixture. However, the question is asking for the amount in moles, so we must round to the correct number of significant figures, which is 2. Therefore, the answer is: 0.0839 mol CO₂.

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