An experiment shows that a 250mL gas sample has a mass of 0.433g at a pressure of 740 mmHg and a temperature of 29 C.

What is the molar mass of the gas?

To find the molar mass of the gas, we can use the ideal gas law equation: PV = nRT.

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's convert the given values into appropriate units:
Volume (V) = 250 mL = 0.25 L (since 1 L = 1000 mL)
Pressure (P) = 740 mmHg
Temperature (T) = 29 °C = 29 + 273.15 K (since temperature must be in Kelvin)

Now we can apply the ideal gas law equation to find the number of moles (n) of the gas:
PV = nRT

n = (PV) / (RT)

n = (740 mmHg * 0.25 L) / (0.0821 L*atm/mol*K * (29 + 273.15) K)
n = (185 mmHg * L) / (24.47 L*mmHg/mol*K)

n ≈ 7.57 mol

Next, we need to find the mass of the gas. We are given that the mass of the gas sample is 0.433 g.

Now we can calculate the molar mass (M) using the equation:
M = mass / moles

M = 0.433 g / 7.57 mol

M ≈ 0.0572 g/mol

Therefore, the molar mass of the gas is approximately 0.0572 g/mol.

Use PV = nRT to determine n.

Then n = grams/molar mass. You know n and grams, calculate molar mass.