Chemical kinetics

2NO (g) + O2 (g) → 2NO2 (g) the following data were obtained for the initial rates of NO consumption.

rate2 rate1 = k[NO]2 x [O2 ]2 y k[NO] 1 x [O2 ] 1 y 0.112M/s 0.0281M/s = k(0.0250M) x (0.0253M) y k(0.0125M) x (0.0253M) y 3.98≈ 4 = 2x so x = 2 0.0281M/s 0.0561M/s = k(0.0125M) x (0.0253M) y k(0.0125M) x (0.0506M) y 0.5 = 0.5y so y = 1 rate = k[NO]2 [O2] = rate [NO] 2 [O2 ] = 0.0561M/s (0.0125M) 2 (0.0506M) = 7.10 ×103 M-2 s -1

. If the rate of appearance of O2 in the reaction: 2O3(g) → 3O2(g) is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?

d[o2]/dt .250x5.50= 1.38 M

HI dissociates to form I2 and H2: 2HI(g) → H2(g) + I2(g) If the concentration of HI changes at a rate of -0.45 M/s, what is the rate of appearance of I2(g)?

usign rate equation -d [HI]/2dt =d[I2]/dt d[I2]/dt =0.45/2=0.225 M/s so C. .23 M/s

HI dissociates to form I2 and H2: 2HI(g) → H2(g) + I2(g) If the concentration of HI changes at a rate of -0.45 M/s, what is the rate of appearance of I2(g)?

d [HI]/2dt =d[I2]/dt d[I2]/dt =0.45/2=0.225 M/s so C. .23 M/s

If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2? N2 (g) + 3 H2 (g) à 2 NH3 (g)

The balanced reaction is : N2 (g) + 3 H2 (g) \rightarrow 2 NH3 (g) Rate of reaction = -\small \Delta[N2]/\small \Deltat = -(1/3) * \small \Delta [H2]/\small \Deltat = (1/2) * \small \Delta [NH3]/\small \Deltat Given : \small \Delta [NH3]/\small \Deltat = 0.345 M/s -\small \Delta[N2]/\small \Deltat = (1/2) * \small \Delta [NH3]/\small \Deltat -\small \Delta[N2]/\small \Deltat = (1/2) * (0.345 M/s) -\small \Delta[N2]/\small \Deltat = 0.1725 M/s Rate of disappearance of N2 = 0.1725 M/s