We can use the ideal gas law to solve for the pressure:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin:
571.7 K = 298.55°C + 273.15 = 871.7 K
Now we can plug in the values and solve for P:
P = nRT/V
P = (1.90 mol)(0.08206 L·atm/mol·K)(871.7 K)/(76.2 L)
P = 37.9 atm
Finally, we convert the pressure from atm to bar by dividing by 1.01325:
P = 37.9 atm / 1.01325 = 37.4 bar
Therefore, the pressure is 37.4 bar when 1.90 moles of an ideal gas occupy 76.2 L at 571.7K.