Acrylonitrile ( C3H3N ) is produced in the following reaction: 2 C3H6 (g) + 2 NH3 (g) + 3 O2 (g) —> 2 C3H3N (g) + 6 H2O (g)
The three reactant gases are mixed in a 150.0 liter reactor at the following partial pressures:
P of C3H6 is 5.00 X 105 Pa
P of NH3 is 8.00 X 105 Pa
P of O2 is 1.50 X 106 Pa
The temperature is 25 degrees C. Calculate the mass of C3H3N that can be produced from this mixture

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole

option c: 1605.1 kj

the balanced chemical reaction for combustion of methane is as follows:

here, enthalpy formation of is -74.7 kj/mol, 0 kj/mol, -393.5 kj/mol and -241.82 kj/mol respectively.

the heat released or can be calculated as follow:

putting the values,

thus, heat released by combustion of 1 mol of methane is 802.54 kj/mol. thus, for 2 mol, heat released will be:

therefore, heat released by the combustion of 2 mol of methane is 1605.1 kj.