Answer :
At 21.0 ºC and a pressure of 757 torr, a gas was found to have a density of 1.64 g L-1. The molar mass of the gas is approximately 36.736 g/mol.
To calculate the molar mass of a gas, we need to use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the temperature from Celsius to Kelvin. We can do this by adding 273.15 to the Celsius temperature:
21.0 ºC + 273.15 = 294.15 K
Next, we can rearrange the ideal gas law equation to solve for n:
n = PV / RT
Given that the pressure is 757 torr and the density is 1.64 g L-1, we can use the relationship between density and molar mass to find the number of moles:
density = molar mass / molar volume
Since the molar volume is equal to 22.4 L at standard temperature and pressure (STP), we can rewrite the equation as:
density = molar mass / 22.4 L
Solving for molar mass:
molar mass = density × 22.4 L
Plugging in the given density of 1.64 g L-1:
molar mass = 1.64 g L-1 × 22.4 L
= 36.736 g
So, the molar mass of the gas is approximately 36.736 g/mol.
You can learn more about molar mass at: brainly.com/question/30640134
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