what is the universal gas constant( the R, in the equation PV=nRT) of this question?
What is the pressure in a 10.0-L cylinder filled with 0.470 mol of nitrogen gas at a temperature of 329 K?
To find the value of the universal gas constant (R), we need to refer to standard reference materials such as chemistry textbooks or online resources. However, I can provide you with the general value of the universal gas constant, which is widely used in various calculations.
The universal gas constant (R) is approximately equal to 8.314 J/(mol·K) or 0.0821 L·atm/(mol·K). The specific value depends on the units of pressure, volume, and temperature used in the equation.
Now, let's calculate the pressure in the 10.0-L cylinder filled with 0.470 mol of nitrogen gas at a temperature of 329 K, using the ideal gas law equation PV = nRT.
In this equation:
P represents the pressure,
V represents the volume,
n represents the number of moles,
R represents the universal gas constant, and
T represents the temperature.
First, we'll rearrange the equation to solve for P:
P = nRT / V
Now, we can substitute the given values into the equation:
P = (0.470 mol) * (8.314 J/(mol·K)) * (329 K) / (10.0 L)
By performing the calculations, we can determine the value of pressure (P) in the cylinder.