If 1.00 L of an unknown gas at STP has a mass of 5.40 g,what is the molar mass?

To find the molar mass, we can use the following formula:

molar mass = (mass of gas) / (number of moles of gas)

At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. We have 1.00 L of the gas. Therefore, we can calculate the number of moles of the gas using:

number of moles = 1.00 L / 22.4 L/mol = 0.0446 mol

Now, we can find the molar mass by plugging values into the formula:

molar mass = 5.40 g / 0.0446 mol = 121.06 g/mol

Therefore, the molar mass of the unknown gas is approximately 121.06 g/mol.

To find the molar mass of the unknown gas, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (STP = 1 atm)
V = volume (1.00 L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (STP = 273.15 K)

First, let's calculate the number of moles of the gas using the ideal gas law equation.
PV = nRT

n = PV / RT

Since the volume is given in liters, pressure is given in atmospheres, and the value of R is 0.0821 L.atm/mol.K, we can calculate the number of moles:

n = (1.00 L * 1.00 atm) / (0.0821 L.atm/mol.K * 273.15 K)

n ≈ 0.0402 mol

Next, we'll calculate the molar mass of the gas using the equation:

Molar mass = mass / moles

Given the mass of the gas is 5.40 g and the number of moles is approximately 0.0402 mol, we can calculate the molar mass:

Molar mass = 5.40 g / 0.0402 mol

Molar mass ≈ 134.33 g/mol

Therefore, the molar mass of the unknown gas is approximately 134.33 g/mol.

To find the molar mass of the unknown gas, we need to use the ideal gas law and the concept of molar mass. The ideal gas law equation is:

PV = nRT

In this equation:
- P represents the pressure of the gas
- V represents the volume of the gas
- n represents the number of moles of the gas
- R is the ideal gas constant
- T represents the temperature of the gas

First, let's break down the given information:

STP (Standard Temperature and Pressure) conditions:
- Temperature (T) is 273.15 Kelvin (0 degrees Celsius)
- Pressure (P) is 1 atmosphere (atm)

We are given:
- Volume (V) is 1.00 L
- Mass of the gas is 5.40 g

To find the molar mass, we'll use the relationship between moles, mass, and molar mass:

moles (n) = mass / molar mass

Now, we can rearrange the ideal gas law equation to solve for moles (n):

n = PV / RT

Substituting the known values:
P = 1 atm
V = 1.00 L
R = 0.0821 L.atm/mol.K (ideal gas constant)
T = 273.15 K (STP temperature)

We can calculate the number of moles:
n = (1 atm * 1.00 L) / (0.0821 L.atm/mol.K * 273.15 K)

Now that we have calculated the number of moles, we can rearrange the equation mentioned earlier to solve for the molar mass:

molar mass = mass / moles

Substituting the known values:
mass = 5.40 g
moles (calculated above)

Calculating the molar mass:
molar mass = 5.40 g / (calculated moles)

By performing these calculations, you will find the molar mass of the unknown gas.