Respuesta :
The molar mass of the gas sample is closest to the molar mass of option (e) SO2, which is 64.07 g/mol. Therefore, the gas sample is likely SO2.
To determine the identity of the gas sample, you can use the ideal gas law, which relates the pressure, volume, temperature, and number of moles of a gas. The ideal gas law can be expressed as:
PV = nRT
where P is the pressure of the gas in units of atm, V is the volume of the gas in liters, n is the number of moles of gas, R is the gas constant (8.31 J/mol*K), and T is the temperature of the gas in Kelvin.
To use this equation, you need to convert the temperature to Kelvin by adding 273.15 to the temperature in Celsius. You also need to convert the pressure from torr to atm by dividing the pressure in torr by 760 (since 1 atm = 760 torr).
Using these conversions, you can plug in the values given in the problem to solve for the number of moles of gas:
P = 790 torr / 760 = 1.03 atm
V = 1.365 L
T = 95 °C + 273.15 = 368.15 K
R = 8.31 J/mol*K
Plugging these values into the ideal gas law equation gives:
1.03 atm * 1.365 L = n * 8.31 J/mol*K * 368.15 K
Solving for n gives:
n = 0.0428 mol
Now that you know the number of moles of gas, you can use the molar mass of each of the gases listed in the options to determine which gas has a molar mass closest to the mass of the sample. The mass of the sample is 3.33 g, so you can calculate the molar mass of the gas by dividing the mass of the sample by the number of moles:
3.33 g / 0.0428 mol = 77.9 g/mol
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