Need help on number 17. Not sure where I messed up
The following initial rate data apply to the reaction below. F_2 (g) + 2CI_2 O(g) rightarrow 2FCIO_2 (g) + CI_2 (g) Which of the following is the rate law (rate equation) for this reaction? A) rate = k[F_2]^2 [CI_2 O]^4 B) rate = k[F_2]^2 [Cl_2 O] C) rate = k[F_2]^2 [Cl_2 O] D) rate = k[F_2][CI_2 O]^2 E) rate = k[F_2] [CI_2 O]^2 The reaction 2NO_2 (g) rightarrow 2NO (g) + O_2 (g) is suspected to be second order in NO_2. Which of the following kinetic plots would be the most useful to confirm whether or not the reaction is second order? A) a plot of [NO_2]^-1 vs. t. B) a plot of ln [NO_2] vs. t C) a plot of [NO_2] vs. t D) a plot of ln[NO_2]^-1 vs. t E) a plot of [NO_2]^2 vs. t If the reaction 2H_2 S (g) 2H_2 (g) is carried out at 1065 degree C, K_p = 0.0120. Starting from pure H_2 S introduced into an evacuated vessel at 1065 degree C, what will the total pressure in the vessel be at equilibrium if the equilibrated mixture contains 0.300 atm of H_2 (g)? A) 0.90 atm B) 0.94 atm C) 1.06 atm D) 1.52 atm E) 1.86 atm
The linearity of each graph can be used to identify the order of a reaction.
Characteristics of second-order reactions
For a second-order reaction, [A]âproducts, the rate of the reaction is given as rate= k[A]2, where k is the rate constant and [A] is the concentration of reactant A. The integrated rate law for second-order reactions is 1[A]t=kt+1[A]0, where [A]t is the concentration of reactant Aat time t, k is the rate constant, and [A]0 is the initial concentration of reactant A. This equation is of the type y=mx+b. Therefore, the plot of 1[A]tversus time is always a straight line with a slope k and a y intercept 1[A]0.
Consider the second-order reaction: 2HI(g)âH2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 7.05Ã1010 s ([HI]t) for a reaction starting under the condition in the simulation?
