For the reaction A +B+ C D E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected Trial A Bl Cl Initial rate 0.30 0.30 0.30 9.0x10 o 2.7x10-4 0.30 0.30 0.90 3.6x10-4 0.60 0.30 0.30 3.6x10-4 0.60 0.60 0.30
What is the value of the rate constant k for this reaction? When entering compound units, indicate multiplication of units explicitly using a multiplication dot (multiplication dot in the menu). For example, M−1⋅s−1. Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.

Rate constant of the reaction is .

Explanation:

A + B + C → D + E

Let the balanced reaction be ;

aA + bB + cC → dD + eE

Expression of rate law of the reaction will be written as:

Rate(R) of the reaction in trail 1 ,when :

...[1]

Rate(R) of the reaction in trail 2 ,when :

...[2]

Rate(R) of the reaction in trail 3 ,when :

...[3]

Rate(R) of the reaction in trail 4 ,when :

...[4]

By [1] ÷ [2], we get value of c ;

c = 1

By [3] ÷ [4], we get value of b ;

b = 0

By [2] ÷ [3], we get value of a ;

a = 2

Rate law of reaction is :

Rate constant of the reaction = k

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