What volume is occupied by 1.00 kg of helium at 5.00 $\circ$ C at a pressure of 735 Torr?

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, and rearranging to solve for V, we get V = nRT/P. We need to find the number of moles, n, of helium first. We can use the molar mass of helium (4.00 g/mol) to convert the mass of 1.00 kg to moles:

n = (1.00 kg)/(4.00 g/mol) = 250 mol

Next, we need to convert the temperature from Celsius to Kelvin:

T = (5.00 °C) + 273 = 278 K

Now we can plug in all the values into the equation:

V = (250 mol)(0.0821 L·atm/mol·K)(278 K)/(735 Torr) = 5.90 x 10^3 L = 5.90 x 10^-3 m^3 = 5.90 m^3

Note: Choice A has an incorrect unit conversion (should be 10^-3 not 10^15), Choice C is half of the correct answer and Choice D is only slightly larger than the volume of 1 mol of gas. Choice E is not consistent with the given parameters.

What Volume Is Occupied by 1 ∘\circ∘ C at a Pressure of 735 Torr? A) 5

What Volume Is Occupied by 1 $\circ$ C at a Pressure of 735 Torr?
A) 5