calculate the pressure,in atmospheres, of 2.00 mol helium gas in a 10.0-L container at 27 celcius?
Use PV = nRT
Note the correct spelling of celsius.
Don't forget to change temperature to Kelvin.
To calculate the pressure of a gas, we can use the Ideal Gas Law, which states that:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles of gas
R is the ideal gas constant
T is the temperature in Kelvin
First, we need to convert the temperature from Celsius to Kelvin. The Kelvin scale starts at absolute zero, which is 0 Kelvin. To convert, we add 273.15 to the Celsius temperature:
27 °C + 273.15 = 300.15 K
Now we can substitute the values into the Ideal Gas Law equation:
P * 10 L = (2.00 mol) * (0.0821 L·atm/(mol·K)) * (300.15 K)
Note: The value for R is 0.0821 L·atm/(mol·K). This is the ideal gas constant in the appropriate units.
Simplifying the equation:
10P = 2 * 0.0821 * 300.15
10P = 49.29
Divide both sides by 10:
P = 4.929 atm
Therefore, the pressure of the 2.00 moles of helium gas in a 10.0-L container at 27 °C is 4.929 atmospheres.