If a certain gas has a density of 2.34 g/L at 27.0C and 742 torr, what is the molar mass of this gas?
I am not sure what formula to use to solve this problem.
To solve this problem, you can use the ideal gas law equation.
The ideal gas law equation is: PV = nRT, where:
P represents the pressure,
V represents the volume,
n represents the number of moles,
R represents the ideal gas constant (0.0821 L·atm/mol·K), and
T represents the temperature in Kelvin.
In this case, you're given the density (g/L), temperature (Celsius), and pressure (torr). However, you need to convert the density to moles per liter to use the ideal gas law equation.
To convert the density to moles per liter, divide the density by the molar mass. The formula for density is defined as:
density = mass / volume
Now, you can rearrange the formula to solve for mass:
mass = density * volume
Substituting the values given:
mass = 2.34 g/L * 1 L
mass = 2.34 g
To convert grams to moles, divide the mass by the molar mass:
moles = mass / molar mass
Rearranging this equation, you get:
molar mass = mass / moles
Now, you have everything you need to find the molar mass. Convert the temperature to Kelvin by adding 273.15 to the Celsius value. Plug in the given values into the ideal gas law equation and solve for the molar mass.