A sample of 1.00 moles of oxygen at 50°C and 98.6 kPa occupies a volume

27.22dm³

Explanation:

Given parameters:

number of moles = 1 mole

temperature  = 50°C, in K gives 50+273 =323K

Pressure  = 98.6kpa in atm, gives 0.973atm

Unknown:

Volume of the gas = ?

Solution:

Since the unknown is the volume of gas, applying the ideal gas law will be appropriate in solving this problem.

The ideal gas law is mathematically expressed as;

            Pv = nRT

where P is the pressure of the gas

          V is the volume

          n is the number of moles

          R is the gas constant

         T is the temperature

Input the parameters and solve for V;

                    0.973 x V  = 1 x 0.082 x 323

                           V  = 27.22dm³

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.