what is the volume occupied by 15.2 g of argon gas at a pressure of 1.04 atm and a temperature of 353 k ?
1 answer:
The volume of argon will be 10.57 L.
Apply the ideal gas law, PV = nRT, where n is the number of moles and R is the gas constant.
We must divide the given mass of argon by its molar mass because we have mass and need moles. Argon has a molar mass of 40 g/mol.
So the number of moles of Argon in 15.2g is = mol
Given:
P = 1.04 atm
n = 0.38 mol
R =
T = 353 K
Unknown:
V
Solution:
V =
V = L
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0.58 is the molarity of 29.9 g of MgS in 911 mL of solution.
Define the molarity of a solution.
Molarity (M) is the amount of a substance in a certain volume of solution. Molarity is defined as the moles of a solute per litres of a solution. Molarity is also known as the molar concentration of a solution.
Given data:
Volume of solution = 911 mL=0.911L
Given the mass of MgS = 29.9 g
Molar mass of MgS = 56.38 g/mol
Moles of MgS = 0.5303299042
Molality = 0.5821403998=0.58
Hence, 0.58 is the molarity of 29.9 g of MgS in 911 mL of solution.
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