The reaction A + B → C+ D rate = k[A][B]² has an initial rate of 0.0640 M/s. What will the initial rate be if [A] is halved and [B] is tripled? initial rate: M/s What will the initial rate be if [A] is tripled and [B] is halved? initial rate: M/s

1) Consider the reaction below. If the concentration of B doubles, what happens to the concentration of A, in the same length of time? 2 A B + 3 C 3 ㅎd[A] doubles triples reduces to one-halfreduces to one-third A -LUCA] = d[B] = 1 A[W) jun 3 =2= 2 dit d+ ↑ dt2) A reaction proceeds during which the half-life of the reactant, A, is shown to increase The rate over time. What is the order with respect to A2 concentrations of A retubes to A? i one warter for ro order realtion not predictable dictory =-4 Rate - +42 = K[AO] +1/2 of 1 САОЈ [A] zeroth first second this is not possible, as half-life would be constant the order is not predictable based on this information A 2 B + C 3) What is the order for the alpha decay of lead-210? All radioactive decay zeroth first second the order is not predictable based on this information quadruples reduces to one-quarter 2 ¿CB] =2 dUB] of zeroth 4) Given the plot below, determine the reaction order for 2 A C. first second d+ reactions are first orter…

A) In the proposed reaction mechanism below, the intermediate product is: A).  NO(g) B).  N2O2(g) C).  H2(g) D).  N2O(g)   B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors  A) 2 B) 3 C) 6 D) 9

The reaction   A+B⟶C+Drate=?[A][B]2A+B⟶C+Drate=�⁡[A]⁢[B]2   has an initial rate of 0.0920 M/s.0.0920 M/s. What will the initial rate be if [A]is halved and [B] is tripled? initial rate: ? M/s What will the initial rate be if [A] is tripled and [B] is halved? initial rate:? M/s

9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I¯(aq). What is the rate law for this reaction? Step 2 (fast) H₂O2(aq) + 10 (aq) → H₂O(l) + O2(g) + (aq) A) rate= K[H₂O₂] B) rate= K[H₂O₂]² C) rate= K[H₂O₂] [1] D) rate = K[H₂O₂] [10] E) rate = K[H₂O₂]²[1]/[H₂O] Tap here or pull up for additional resources 36% Submit

For the multi-step reaction A +B C+D the rate-limiting step is unimolecular, with A as the sole reactant. If [A] and [B] are both 0.110 M, then the rate of reaction is 0.0020 M/s. What is the rate of the reaction if [A] is doubled? rate: M/s Starting with the original concentrations, what is the rate of the reaction if [B] is doubled? rate: M/s Starting with the original concentrations, what is the rate of the reaction if [A] and [B] are both increased by a factor of 3? rate: M/s

Consider the reaction and its rate law. 4A + 3B What is the order with respect to A? order: products What is the order with respect to B? order: What is the overall reaction order? overall order: rate = k[A]²[B]²

It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s

* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit

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