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 #at the bottom}3,17g/mole contained in a 4.00 flask at 32.5 degrees Celsius and 1.6atm?
To solve this problem, you can use the ideal gas law equation, which is PV = nRT, where P represents the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, let's rearrange the ideal gas law to solve for the number of moles (n):
n = PV / RT
We are given:
- Pressure (P) = 1.6 atm
- Volume (V) = 4.00 L
- Temperature (T) = 32.5 degrees Celsius
Before we proceed with the calculations, we need to convert the temperature to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 32.5 + 273.15
T(K) ≈ 305.65 K
Now, let's calculate the number of moles (n):
n = (1.6 atm * 4.00 L) / (0.0821 L•atm/(mol•K) * 305.65 K)
n ≈ 0.255 moles
To determine the mass of ammonia gas, we need to convert the number of moles to grams using the molar mass of ammonia (NH₃), which is approximately 17 grams/mole.
Mass = moles * molar mass
Mass ≈ 0.255 moles * 17 grams/mole
Mass ≈ 4.335 grams
Therefore, the mass of ammonia gas in the 4.00 L flask at 32.5 degrees Celsius and 1.6 atm is approximately 4.335 grams.