For a hypothetical reaction: A + 2B + C → D + E The rate law has been determined and is as follows: Rate = k[A][B]2 What happens to the reaction rate when we make each of the following concentration changes? a) We triple the concentrations of A, B and C simultaneously. b) We triple the concentration of D

NTERACTIVE EXAMPLE Reaction Rate Chloromethane reacts with iodide ion to yield iodomethane and chloride ion. CH;C1 +r- CH;I + CF A way to determine the rate of the reaction of chloromethane with iodide ion is to measure the disappearance of T from the solution. Suppose that the concentration of I was 0.21 mol IL at the start of the reaction. At the end of 20 min, the concentration dropped to 0.13 mol L. This difference is equal to a change in concentration of -0.08 mol IL. QUESTION What is the rate of reaction with respect to iodide ion? |× molIL'min

The reaction rate of CO and NO2 in the reaction   CO(g) + NO2(g) → CO2(g) + NO(g)   is measured using the initial rates method. The results are tabulated below. [CO] (mol/L)   NO2 (mol/L)   -([CO]/Δt (mol/L·s) 8.00 10-4   5.50 10-4   8.40 10-8 8.00 10-4   7.78 10-4   1.68 10-7 1.60 10-3   5.50 10-4   1.68 10-7             Determine the rate expression and calculate the rate constant for the reaction.

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.

The following exothermic reaction is at 0.00 °C and 1.00 atm       SeO­4 (g) ⇌   Se(g) + O2(g)   , kc = 2.4 ×10-6 The reaction contains [SeO4] = 0.100 M, [Se] = 0.0034 M, [O2] = 0.0022 MWhat will happen to the rate of the reaction if the concentration of SeO4 is increased by 10 times?

R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³

please answer both please i will upvote ( if you have plan to answer only one then please skip , let someone accept the question who can do both )

6. The gas phase reaction A+B C has a reaction rate which is experimentally observed to follow the relationship rate= k[A]2[B]. Which one of the following would affect the value of the specific rate constant, k? (a) increasing the temperature(b) changing the concentration of A (c) changing the concentration of B(d) changing the concentration of C (e) all of the above

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Second Year Second Semester 2018-2019 First Month Exam School of Chemistry Organic Chemistry QI/ Consider the following reaction: "OCICH,, Br (CH,,COH ン しい」 What happens to the reaction rate guh each of the following changes? is (1) The concentration of OC(CH is decreased.(2) The base is changed to "OH. (3) The halide is changed to CH;CH:CH2CH,CH(Br)CH3. (4) The leaving group is changed to I.