What pressure will be exerted by 0.57 moles of CO2 at a temperature of 25°C and a volume of 500 ML? atm

The pressure exerted by 0.57 moles of CO2 at a temperature of 25°C and a volume of 500 ml is 28 atm.

Explanation:

According to ideal gas law,

                                      PV = nRT

where P represents the pressure of a gas,

          V  represents the volume of a gas,

          n represents the number of moles,

          R represents the gas constant = 0.0821 L atm / mol K.

          T represents the temperature of a gas.

Given V = 500 ml = 0.5 l,           T = 25°C = 298 K,   n = 0.57 mol

                                        PV = nRT

                                           P = nRT / V

                                              = (0.57 0.0821 298) / 0.5

                                          P = 28 atm.

The pressure of a gas is 28 atm.

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c. 4.54 x 10–12 j happens to be correct