Question

Given that the rate constant for the decomposition of hypothetical compound X from part A is 1.60 M−1⋅min−1, calculate the concentration of X after 18.0 min .

X(g)⇌Y(g)+Z(g)

Time (min)	[X](M)
0	0.467
1	0.267
2	0.187
3	0.144
4	0.117
5	0.099
6	0.085
7	0.075

Answer 1

The decomposition of the compound is given as - x(9) Y (9) + 2(g) The nate constant is given = 1.6 M miñ = 16 (modit") min! = 16 L moi mint The general formula to determine the unit of k is – 9ъ thе еасhion odor 5т деп (1-n) (n-1) - unit of k= mol L time The K e given = 1.6 L. moe! mins so clearly at the order of reaction ý 2 as, n-1=1 n=2 This is a 2nd order reation. The general formula of rate of a and order reaction h - kt- ala-x) k= rate constant, t= time

a= initial concentration of product x= concentration after time t a= initial concentration given = 0.467 (M) at omin so, t= K= x= ?? 18 min 16 ml min! kta ala-x) or 1.6 mo man x 18 shin = 0.467 0 (0.467 m-x) or (0.467 m-x) = 13.4496 113.4496% 0.467 or x = 14.4496 2 0.434 M after of 18 min product the concentration will be = 0.434 (M) i concentration of x after 18 min - (0.467-0.434) (M) - 0.033(M)