Practice ProblemBUILD
Write the balanced equation corresponding to the following rate expressions:
(a)
rate =
(b)
Rate =
(c)
rate =
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- Write the rate equation for each of the following elementary reactions:(a) O3 ⎯⎯⎯⎯⎯⎯⎯→ sunlight O2 + O(b) O3 + Cl ⟶ O2 + ClO(c) ClO + O ⟶ Cl + O2(d) O3 + NO ⟶ NO2 + O2(e) NO2 + O ⟶ NO + O2arrow_forwardCurrent Attempt in Progress The reaction 2A + 2B M+Nhas the rate law: Rate = k[A]?. At 25°C, k = 0.0376 L mol1s1. If the initial concentrations of A and B are 0.387 M and O.459 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 68.7 seconds Hint Your answer is incorrect. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = i ! M [B] = i M Hintarrow_forwardThe reaction, A + 2 B → products, has the rate law, rate = k(A)2(B)1. When the concentration of A is tripled, while that of B doubled, by what factor will the rate of the reaction increase? (A) 5 (B) 24 (C) 12 (D) 18 (E) 6arrow_forward
- For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) (a) rate = k (X][Y][Z]² X Y Overall rate = k (X]/[Y]/² [Z] -1 (b) 1/2 X Y Overall (c) rate = k [Y] X Y Overallarrow_forwardFor a reaction that follows the general rate law, Rate = k[A]0[B]3, what will happen to the rate of reaction if theconcentration of A is tripled and the concentration of B is doubled?(a) Increase by a factor of 6(b) Increase by a factor of 8(c) Increase by a factor of 9(d) Increase by a factor of 12arrow_forwardSulfur dioxide emissions from power plants reacts with carbon monoxide as follows: SO2(g) + 3 CO(g) → 2 CO2(g) + COS(g)If the average rate of consumption of CO is 0.38 M/s, what is the rate of formation of CO2(g)?(a) 0.25 M/s(b) 0.57 M/s(c) ‒0.25 M/s(d) ‒0.57 M/sarrow_forward
- If the rate law for the reaction A ⟶Products is rate = k[A], calculate the value of k from the following data: [A] (M) Initial Rate (M/s) 0.10 0.015 (A)6.7 s-1 (B)0.015 s-1 (C)0.15 s-1 (D)67 s-1arrow_forwardWhich of the following could be the instantaneous rate ofthe reaction in Figure 14.3 at t = 1000 s?(a) 1.2 x10-4 M>s(b) 8.8 x 10-5 M>s(c) 6.3 x 10-5 M>s(d) 2.7 x 10-5 M>s(e) More than one of these.arrow_forwardDetermine (a) the rate equation and (b) the rate constant for the hypothetical reaction A + B ® C given the following initial concentrations and initial rate data. [A]0 [B]0 Initial Rate Run # (mol/L) (mol/L) (mol/L·s) (1) 0.100 0.100 0.18 (2) 0.100 0.200 0.36 (3) 0.200 0.200 1.44arrow_forward
- At a certain concentration of reactants the rate of appearance of water in the following reaction is 0.73 M/s. HINT: Watch the sign of the rate! 4NH3 + 70₂ → 4NO₂ + 6H₂O X M/s (A) What is the rate of reaction of O₂? [0.30 (B) What is the rate of reaction of NH3? 0.17 (C) What is the rate of reaction of NO₂? 0.29 X M/s X M/sarrow_forward3. What is the half-life of a first order process with a rate constant of 4.50 x 10´³ s¯¹? Cannot be determined given this information. (A) (B) -3 6.49 x 10 s (C) 66.9 s (D) 15.4 s (E) 154 sarrow_forward36) The following graph shows the kinetics curves for the reaction of oxygen with hydrogen to form water: O,lg) + 2H;(g) → 2H,0(g). Which curve is Oxygen? dashed gray black a) the dashed curve c). either the gray or the black curve b) the gray curve d) the black curvearrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax