so here i am doing my hw worksheet on the ideal gas law/ghram's law ad i have gotten to this one problem where i am totally stuck and confused. Please help me by telling me how to set this up and giving me tips, if necessary.
What is the mass(in grams) of ammonia gas(NH{tiny #3at the bottom},17g/mole contained in a 4.00 flask at 32.5 degrees Celsius and 1.6atm?
PV = nRT
P = 1.6 atm
V = 4.00 L or whatever unit you didn't type in.
R = 0.08206 L-atm.
T = 273 + 32.5 = ??K
n = solve for this.
Then n = grams/molar mass
You know n from above, grams is what you want and molar mass NH3 = 17 g/mole.
To solve this problem using the ideal gas law, we will use the formula:
PV = nRT
P represents pressure, V represents volume, n represents the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the given temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius value. In this case, 32.5 degrees Celsius is equal to 32.5 + 273.15 = 305.65 Kelvin.
Next, we need to rearrange the ideal gas law to solve for the number of moles:
n = PV / RT
Given that the pressure is 1.6 atm, the volume is 4.00 L, the temperature is 305.65 K, and the gas constant is R = 0.0821 L·atm/(mol·K), we can substitute these values into the equation to calculate the number of moles.
n = (1.6 atm) * (4.00 L) / (0.0821 L·atm/(mol·K) * 305.65 K)
n = 0.0836 mol
Now that we have the number of moles, we can calculate the mass by using the molar mass of ammonia (NH₃), which is 17 g/mol.
Mass = number of moles * molar mass
Mass = 0.0836 mol * 17 g/mol
Mass = 1.4192 g
Therefore, the mass of ammonia gas contained in the 4.00 L flask at 32.5 degrees Celsius and 1.6 atm is approximately 1.4192 grams.