Ap Chemistry

posted by .

Hi, I was wondering if you could possibly help me with this chem question.

For the relatively slow decomposition of NOCL into NO and Cl2 according to the reaction below, it is known that the reaction is second order w/ respect to NOCl and that after 23.4 minutes that 75% of NOCl is decomposed when the initial concentration of NOCl is 0.0732 M. How long (in minutes) would it take until 35.8% of the NOCl has decayed?

2 NOCl ---> 2 NO + Cl2

i think i have to use the integrated law but other than that how would i work this out? Thank you.

1/[A]=(kt + 1)/A null

• Ap Chemistry -

For a second order reaction, the equation is
(1/A) - (1/Ao) = akt
I think you have Ao, A, a, and t (23.4 min) so you can solve for k (at 75% decomposition).
Then use k in the revised equation. You will have k, A, Ao (for 35.8% decomposition) and a, and you can solve for t. Check my thinking.

Similar Questions

1. Chem II

2.5 mol NOCl(g) was placed in a 2.50 L reaction vessel at 400 degrees C. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation: 2NOCl(g)<-->2NO(g)+Cl2(g) Calculate the …
2. chemplz

At 462degrees, the reaction (1) heat + 2 NOCl(g) <=====> 2 NO(g) + Cl2(g) has an equilibrium constant, Keq = 8.0 x 10-2. a) What is Keq at 462degrees for the reaction 2 NO(g) + Cl2(g) <=====> 2 NOCl(g) 1/Keq may I ask how …
3. chemistry

I also had a problem with this type of questionthe initial pressure of NOCl(g) is 4.329 atm, calculate the % of NOCl(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 400.0 °C …
4. Chemistry

At 35 degrees Celcius, K = 1.6x10^-5 for the reaction: 2NOCl<--> 2NO + Cl2 If 2.0mol NOCl and 1.0mol Cl2 are placed into a 1.0-L flask, calculate the equilibrium concentrations of all species. Answer: [NOCl] = 2.0M [NO] = 8.0x10^-3 …
5. chemistry

I have been at this question for at least three hours now. Consider the chemical system below. 2 NOCl(g) 2 NO(g) + Cl2(g) K = 1.6 10-5 What is the equilibrium concentration of nitrogen monoxide, [NO], given each of these initial conditions?
6. Chemistry

The following reaction exhibits the rate law: Rate = k[NO2]^2[Cl2]. 2NO(g)+Cl2(g)---->2NOCl (g) (a) Explain why the following mechanism is not plausible for this reaction. Fast: NO + Cl2<-->NOCl + Cl Slow: NO + Cl---->NOCl …