Practice ProblemBUILD
Write the balanced equation corresponding to the following rate expressions:
(a)
rate =
(b)
Rate =
(c)
rate =
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Chemistry
- 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_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_forwardThe half-life of a first-order process is 1.39×10-2 seconds. What is the corresponding rate constant? (A) 50 s-1 (B) 100 s-1 (C) 0.144 s-1 (D) 10-2 S-1 (E) 6.93×10-35-1arrow_forward
- Current 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_forwardConsider the energy diagram shown below for the reaction of A + B → D: A* C D E (a) rate= k[B] k[A] k[D] (d) rate = k[A][C] (e) rate= k[A][B] O (b) rate = O (c) rate = A Reaction Progress Which of the following would be the rate law for this reaction? A A* + B сarrow_forward6. The rate constant for the first-order decomposition of N₂O5 is 6.2 x 10-5s-¹. What is the half- life? (a) 8.9 x 10-5 s (b) 1.1 x 104 s (c) 1.5 x 10³ s (d) 4.5 x 104 sarrow_forward
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- Determine (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_forwardAt 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_forward
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