A 2.8 gram sample of a gaseous substance
occupies 12 L at 47 degrees C and 683 torr. What is the density of the gas under these conditions?
Answer in units of g/L
You can add the PV = nRT equation to the density and come up with
P*molar mass = density*RT
To find the density of the gas, we need to use 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, and T is the temperature. We can rearrange the equation to solve for density (D) by dividing both sides of the equation by V:
D = nRT / V
Now, let's break down the information given in the question:
Mass of the sample = 2.8 grams
Volume (V) = 12 L
Temperature (T) = 47 degrees C (Convert to Kelvin: T = 47 + 273.15 = 320.15 K)
Pressure (P) = 683 torr (Convert to atm: P = 683 / 760 = 0.898 atm)
To find the number of moles (n) of the gas, we need to use the molar mass (M) of the gas. However, you haven't provided the molar mass of the gas in the question, so we can't calculate the number of moles and, subsequently, the density of the gas.
Please provide the molar mass of the gas, and I'll be able to help you find the density.