Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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a.
What is the overall reaction?
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b. Identify any intermediates:
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C.
How many transition states are there?
d. Is step 2 exothermic or endothermic?
e. Is the overall reaction exothermic or endothermic?
> Spacing
1.0 -
f. Which step has the smallest energy of activation associated with it?
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i. What is the value associated with it?
g. Which step is the slowest?
h. What is the rate law for the slowest step?
i.
List two ways you could make the forward reaction go faster.
Potential Eneray (k)
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- Analyze the following reaction mechanism: H2O + O → CIÓ + CF2CI CI + 202 4. Cl + CF2CI –→ CF2CI2 1. H2O2 2. O + CF2CI2 3. CIO + Oз -> Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF;CI, CF2CI2 C) O, CIO, O, H20 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF;CI2arrow_forward4. Consider the following 3 step reaction mechanism: Step 1 H₂ 2H fast Step 2 Step 3 H + HCO H + CO a. What is the overall reaction? HCO slow H₂CO fast b. Identify the intermediates in the reaction mechanism. c. Write a rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.arrow_forward7arrow_forward
- What is the correct rate law for this reaction A(g) + 2B(g) -> 2C(g) + 2D(g)arrow_forwardArrange the following reactions in order of increasing rate (slowest to fastest) i. CzsHs2 (s) + 38 O2 (8) → 5 CO2 (g) + 26 H20 () ii. Ag* (aq) + I'(aq) > Agl (s) iii. H2 (g) + % O2 (8) → H20 a. i, ii, ii b. iii, ii, i c. ii, i, ii d. ii, i, iii e. ii, ii, iarrow_forwardThe rate law of the following reaction is : CH.CH-Br+ OH → CHCH-CH+Br A. Rate= k[CH,CH,-Br] B. Rate = k(CHCH-Br][OH] C. Rate = k(OH] D. Rate= kCHCH-Br][OHT %3D O Darrow_forward
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