1.9 mol of gas at a temperature of -180 C fills a 3.4 L container.
What is the gas pressure?
Never been good at physics or mol stuff, how do you set it up?
Use the ideal gas formula:
P V = n R T
T has to be in Kelvin degrees, which would be 93 K.
n = 1.9 moles
V = 3.4 liters
R = 0.0821 atm*L/mole*K is the "gas constant"
Solve for P in atmospheres
Thank you! That really helped!
You're welcome. Remembering the formula is easy, but I always have to look up the value of R.
To solve this problem, you need to use the ideal gas law equation, which is:
PV = nRT
Where:
P = gas pressure (in units of pressure, such as atmospheres)
V = volume of the gas (in units of liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature of the gas (in units of Kelvin)
Given that you have 1.9 moles of gas, a temperature of -180 °C, and a volume of 3.4 liters, you can follow these steps to calculate the gas pressure:
1. Convert the temperature from Celsius to Kelvin:
- Add 273.15 to the temperature in Celsius to get the temperature in Kelvin.
- In this case, -180 °C + 273.15 = 93.15 K.
2. Use the ideal gas law equation to solve for pressure:
- Rearrange the equation to solve for P: P = nRT/V.
- Plug in the values for n, R, T, and V:
P = (1.9 mol) * (0.0821 L·atm/mol·K) * (93.15 K) / (3.4 L).
- Calculate:
P = 5.08 atm.
Therefore, the gas pressure in the 3.4 L container is 5.08 atm.