A quantity of 2.00 mol of an ideal gas is maintained at a temperature of 127ûC in a containerof volume 0.083 m3 . What is the pressure of the gas?

To solve this problem, we will use the ideal gas law equation, which is PV = nRT.

Here's the step-by-step solution:

1. First, we need to convert the temperature from Celsius to Kelvin because the ideal gas law requires the temperature to be in Kelvin. The conversion formula is K = C + 273.15. So, 127°C = 127 + 273.15 = 400.15 K.

2. Next, we plug the given values into the ideal gas law equation. The number of moles (n) is 2.00 mol, the volume (V) is 0.083 m^3, and the temperature (T) is 400.15 K. The ideal gas constant (R) is 8.314 J/(mol·K) when the volume is in m^3.

3. So, the equation becomes P = nRT/V = (2.00 mol * 8.314 J/(mol·K) * 400.15 K) / 0.083 m^3.

4. Solving this equation gives us the pressure (P) in Pascals (Pa).

Remember to always check your units to make sure they are consistent throughout the problem.