Asample of no2(g) is initially placed in a 2.50-l reaction vessel at 300°c. if the half-life and the rate constant at 300°c are 11 seconds and 0.54 m-1 s-1, respectively, how many moles of no2 were in the original sample? nitrogen dioxide decomposes at 300°c via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation. 2 no2(g) → 2 no(g) + o2(g). a sample of no2(g) is initially placed in a 2.50-l reaction vessel at 300°c. if the half-life and the rate constant at 300°c are 11 seconds and 0.54 m-1 s-1, respectively, how many moles of no2 were in the original sample? 0.17 mol 15 mol 0.42 mol 5.9 mol

58750.08068 is the answer i think

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

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explanation:

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