For the reaction,2COF_2(g) = CO_2(g) + CF_2(g),K_2.00 at a particular temperatur

Question

For the reaction,2COF_2(g) = CO_2(g) + CF_2(g),K_2.00 at a particular temperature.A reaction mixture at this temperature initially contains all three gases in equal concentrations.Which of this reaction mixture.? (A) Q K;the reaction proceeds toward the reactants The reaction A rightarrow products obeys second order kinetics. What is the molar concentration of A remaining after 2.00 minutes if the reactionhas a rate constant of 0.0482 M^1 S^-1and the initial concentration of A is 0.379 M. (A) 0 0655 M (B) 0.119 M(C) 0.366 M(D) 8.42 M Determine the reaction order with respect to [A] for the reaction A + B + C rightarrow products (A) 0 (B) 1 (C) 1.5 (D) 2 According to the collision theory for chemical reaction, why do most reaction rates increase as temperature is increased? At higher temperatures (A) the concentration of reactants increases. (B) the activation energy of the reaction decreases. (C) more molecules collide with the necessary energy. (D) more molecules have the proper orientation when they collide. A chemical reaction is performed at 200 K and at 400 K. The reaction has activation energy of 500 kJ mol^-1 At 400 K the rate of reaction is (A) the same as the rate at 200 K. (B) approximately double the rate at 200 K. (C) approximately 200 times the rate at 200 K. (D) over 3 million times the rate at 200 K. A drug is a in a first order reaction which a bold life of 4.12days.if is a percent 100.0 of this drug what mass reaction after 30.0 days?(A) 0.391 mg (B)0.441 mg (C)0.643 mg (D)0.672 mg The reaction HNC(g) rightarrow HCN(g) is first order is [HNC]which plot is correct for this reaction? Consider this reaction mechanism: The overall reaction is___order with respect to NO_2 and____order with respect toCl_2- (A)2^ml, 2^nl (B) 2^ml,1^m (C) 1^m, 2^ml (D) 1^m, 1^m Which energy diagram best if reaction that is forward best slow?

Explanation / Answer

You have too many questions in the same post. Try to post your questions in different post (no more than two or three questions) in that way you will get answered faster and better.

In this occasion, I will answer three of your questions, and the other post them in another question thread:

33. If this obeys a second order kinetics then the equation to use is: 1/A = 1/Ao + kt. So replacing the given values we have:

1/A = 1/0.379 + 0.0482*(2*60)
1/A = 8.4225
A = 0.1187 M or 0.119 M

34. The general rate law for this reaction would be: rate = k[A]x[B]y[C]z. The product is not taking account in the expression. In order to determine the reaction order of A, we need to take two values of rate where concentration of B and C are constant. The third and fourth trial fullfil this so:

rate 3 = 2.4x104 = k(0.2)x(0.2)y(0.2)z
rate 4 = 2.4x104 = k(0.1)x(0.2)y(0.2)z

rate3/rate4 = 1 = (0.2/0.1)x
1 = 2x
20 = 1 = 2x
x = 0

Question 37.
Calculate the decay constant:
k = ln2/t1/2 = ln2 / 4.12 = 0.168 day-1

m = mo exp(-kt)
m = 100 exp(-0.168*30)
m = 6.43 mg

Hope this helps

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