calculate the pressure,in atmospheres, of 2.00 mol helium gas in a 10.0-L container at 27 celcius?
answered above. Use PV = nRT
To calculate the pressure of a gas, you can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
To calculate the pressure, we need to convert the temperature from Celsius to Kelvin. The Kelvin temperature is equal to Celsius temperature plus 273.15. So, 27 degrees Celsius is equal to 27 + 273.15 = 300.15 Kelvin.
Now we have all the values needed to calculate the pressure. Substitute the values into the ideal gas law equation:
P(10.0 L) = (2.00 mol)(0.0821 L·atm/(mol·K))(300.15 K)
Solving for P:
P = (2.00 mol)(0.0821 L·atm/(mol·K))(300.15 K) / (10.0 L)
P = 4.0937 atm
Therefore, the pressure of 2.00 mol of helium gas in a 10.0-L container at 27 degrees Celsius is approximately 4.0937 atmospheres.