How many moles of argon gas are present in 70L of volume with a pressure of 180atm at 21C?
PV = nRT
To calculate the number of moles of argon gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature (in Kelvin)
First, let's convert the temperature from Celsius to Kelvin. The Kelvin temperature (TK) is equal to the Celsius temperature (TC) plus 273.15:
TK = TC + 273.15
Given that the temperature is 21°C, we can convert it to Kelvin:
TK = 21°C + 273.15 = 294.15 K
Now, we have the following values:
P = 180 atm
V = 70 L
T = 294.15 K
R = 0.0821 L·atm/mol·K
Plug these values into the ideal gas law equation and solve for n:
PV = nRT
(180 atm)(70 L) = n(0.0821 L·atm/mol·K)(294.15 K)
Rearrange the equation to solve for n:
n = (180 atm * 70 L) / (0.0821 L·atm/mol·K * 294.15 K)
n = 12.870 moles
Therefore, there are approximately 12.870 moles of argon gas present in a volume of 70 liters with a pressure of 180 atm at 21°C.