A volume of 0.285 L of a gas at STP weighs 0.537 g. Calculate the molar mass of the gas
(1)(0.285) = n(0.0821)(273).
.0036
is this correct?
no. The number of moles may be .0036.
molmass=grams/numbermoles
so it would be
(1)(.0036)=n(.0821)(273)?
Do you know what a mole is?
You solve PV = nRT for n which gives moles. Then moles = grams/molar mass and solve for molar mass.
To calculate the molar mass of the gas, we need to first determine the number of moles of the gas using 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 (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.
Since the gas is at STP (Standard Temperature and Pressure), we know that the pressure (P) is 1 atm and the temperature (T) is 273 K. Given that the volume (V) of the gas is 0.285 L, we can rearrange the equation to solve for the number of moles (n):
n = (PV) / (RT)
Plugging in the values, we have:
n = (1 atm * 0.285 L) / (0.0821 L·atm/(mol·K) * 273 K)
Simplifying this expression gives:
n = 1.10 mol
Next, we can calculate the molar mass (M) of the gas using the equation:
M = (mass of the gas) / (n)
Given that the mass of the gas is 0.537 g and the number of moles is 1.10 mol, we can substitute these values into the equation:
M = 0.537 g / 1.10 mol
Simplifying this expression gives:
M ≈ 0.488 g/mol
So, the molar mass of the gas is approximately 0.488 g/mol.
Therefore, the answer of 0.0036 is not correct. The correct molar mass is approximately 0.488 g/mol.