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- A + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction. Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2 assuming c is psuedo-state-concentration overall chemical rxn is 3A+2B->2DHi, 40) The rate of a particular reaction doubles when the termperature increases from 25oC to 35oC. Explain why this happens. Thanks,Is the proposed mechanism below valid or invalid? Justify your answer.Overall reaction: 2NO2(g) + F2(g) → 2NO2F(g) ________________________________________________Step 1: NO2(g) + F2(g) →NO2F(g) + F(g) slow Step 2: F(g) + NO2(g) → NO2F(g) fast
- Table 1 with temperature and rate constants Temperature (oC) Rate constants KH (min-1) 61.0 7.13*10-6 71.2 2.77*10-5 Mark and Anthony have considered the following reaction for urea NH2CONH2 in 0.1M HCl: NH2CONH2 + 2H2O --> 2NH+2 + CO2-3 and the rate constant for the reaction is k1. Stephan and Kurt have been in the laboratory and measured rate constants for the reaction at two different temperatures. The measurement results are given in Table 1. 1) You must write down expressions for the changes in time for the concentrations of the reactants and products. That is, determine d[X]/dt, where [X] is the concentration of either reactants or products and write this down using concentrations and the rate constant. 2) You must use the Arrhenius expression to determine the activation energy for the reaction. 3) You must use the Arrhenius expression to determine the pre-exponential factor in the Arrhenius expression.. The proposed reaction mechanism is as follows:i. BrO3- (aq) + H+ (aq) à HBrO3 (aq) [Fast]ii. HBrO3 (aq) + H+ (aq) à H2BrO3+ (aq) [Medium]iii. H2BrO3+ (aq) + Br- (aq) à Br2O2 (aq) + H2O (ℓ) [Slow]iv. Br2O2 (aq) + 4H+(aq) + 4Br-(aq) à 3Br2 (ℓ) + H2O (ℓ) [Fast]Evaluate the validity of this proposed reaction. Justify your answer.The proposed reaction mechanism is as follows:i. BrO3- (aq) + H+ (aq) = HBrO3 (aq) [Fast]ii. HBrO3 (aq) + H+ (aq) = H2BrO3+ (aq) [Medium]iii. H2BrO3+ (aq) + Br- (aq) = Br2O2 (aq) + H2O (ℓ) [Slow]iv. Br2O2 (aq) + 4H+(aq) + 4Br-(aq) = 3Br2 (ℓ) + H2O (ℓ) [Fast]Evaluate the validity of this proposed reaction. Justify your answer.
- What is the unit for rate constant of reaction: A+B --> C 1st order for A and B Rate of rxn = 3.0M/minRank the following in order of increasing rate in a unimolecular reaction. (1=slowest ... 3=fastest)rate law for hte reaction : RX + H20→ R0H + HX , rate =K[RX]. the rate of reaction will be doubled when: (a) concentration of H2O is doubled (b)concentration of RX is reduced to half (c) concentration of RX is doubled (d) none of these also give reason for your answer
- If 75% of a first order reaction was completed in 60 minutes , 50% of the same reaction under the same conditions would be completed in 30 mins. TRUE OR FALSE?Note: Use k to represent the rate constant and place brackets [ ] arounds the molecular or atomic formula to designate concentration. Do not include spaces anywhere in your answers. The rate triples when [BrO] triples. When [BrO] is halved, the rate decreases by a factor of 4. The rate is unchanged when [BrO] is tripled.A2 Please write down the reaction mechanism