At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must be added at constant temperature and pressure if you need a total of 1.48 mol of oxygen gas in the vessel?
Express the volume to three significant figures, and include the appropriate units.
Answer (3)
We first consider the ideal gas equation,
PV = nRT
It is stated that the pressure and temperature are constant; moreover, R is already a constant. So, we get: V = constant * n This is the equation of direct proportion. Therefore, we get:
V/n = constant
V₁/n₁ = V₂/n₂
Substitute the values and solve for V₂
V₂ = (4 * 1.48) / 0.864 V₂ = 6.85
6.85 Liters of gas must be present at the end, so we need to add: 6.85 - 4 = 2.85 liters
To find the** volume of oxygen gas** that needs to be added, we can use the equation: V1 * n1 = V2 * n2. Plugging in the given values, we find that you must add **approximately 2.326 liters **of oxygen gas to the vessel. ;
To reach a total of 1.48 moles of oxygen gas, 2.84 liters must be added to the vessel. The calculation is based on the direct relationship between volume and the number of moles under constant temperature and pressure. Using the formula V₁/n₁ = V₂/n₂, the final volume was determined to be 6.84 L, leading to the conclusion that 2.84 L needs to be added.
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