A 2.0 L sample at 20°C and 750 torr contains 0.5moles of a gas. If 0.1 mole of the gas at the same temperature and pressure is added to the sample, what is the new volume of the gass
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A 2.0 L sample at 20°C and 750 torr contains 0.5moles of a gas. If 0.1 mole of the gas at the same temperature and pressure is added to the sample, what is the new volume of the gass
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Answer:
The new volume of the gas is 1.78 L
Explanation:
The relationship between the number of moles of gas, its pressure, volume, and temperature is given by the Ideal Gas Law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin.
We know that the initial conditions of the gas sample are:
V = 2.0 L
n = 0.5 moles
P = 750 torr = 750 * 1/760 atm = 0.9868 atm
T = 20°C = 293.15 K
After 0.1 mole of gas is added, the new conditions are:
V = ?
n = 0.5 moles + 0.1 moles = 0.6 moles
P = 0.9868 atm
T = 293.15 K
We can use the Ideal Gas Law to find the new volume:
V = (nRT) / P = (0.6 moles * 0.08206 L atm mol-1 K-1 * 293.15 K) / 0.9868 atm = 1.78 L
So, the new volume of the gas is 1.78 L. I hope this has answered your question. Please give a heart if it has. Thank you!!