Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Some measurements of the initial rate of a certain reaction are given in the table below. [N] 0.815M1.56M N,|H||initial rate of reaction 185. M/s 141.M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. 口 rate = 0 ロ || = 1 Explanation Check D2022 McGrny Hl LLC. Al Rights Reserved. Terms of N 回 至 五arrow_forwardA zero order reaction has a constant rate of 3.1 × 10−4 mol·L−1·s−1. If after 60 seconds the concentration has dropped to 4.7 × 10−2 mol·L−1, what was the initial concentration (in mol·L−1)? Express your answer to two significant figures.arrow_forwardA substance containing dye decomposes very quickly. The graphs below were constructed with data pertaining to changes in [dye] over time. The initial concentration of dye was 1.0 M. After 20 seconds passed the concentration of dye was measured to be 0.13 M. [Dye] (mM) 10 00 0.9 -0.5 0.8 0.7 0.6 0.5 0.4 In([Dye]) In(mM) 6 -1 -1.5 1/[Dye] (1/mM) m 0.3 -2 2 0.2 0.1 -2.5 0 10 20 0 10 20 10 20 time (sec) time (sec) time (sec) 1. What is the order for the overall reaction? Justify your answer. Your answer *arrow_forward
- The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?arrow_forwardA certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% Varrow_forwardConsider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)arrow_forward
- Write the reaction rate expressions for the reaction below in terms of the disappearance of the reactants and the appearance of products. Give the expressions for the disappearance of the reactants first, in the order written in the chemical equation. Then write the expressions for the appearance of the products in the order written in the chemical equation. Write the expressions in order of appearance in the equation in the form. where + is either a plus OR a minus sign, not both, X is an integer, and A is a chemical species. Do not include the state of matter. 1 A[4] X At 2H2(g) + O,(g) → 2H,O(g) 1 The rate = At At Atarrow_forwardAluminum will slowly react with oxygen to produce aluminum oxide. The rate of this reaction has been measured for two different reaction conditions. The rate is 4 mmol/s when 2 M Al is reacted with 3 M O, and the rate is 2 mmol/s when 1 M Al is reacted with 3 M O. What would be the value of M for the rate equation, rate = k [Al]^m[O}^narrow_forward(#28) Reaction Rates and time. A decomposition reaction in the first order has a rate constant of 1.26 x 10-4/sec. If the initial concentration of the reactant is 0.644 M. how much time will it take before 20% of the reactant has decomposed? 28a) In blank #1, type-in the working formula to solve for the time required. Enter the algebraic formula as a one-line equation and without spaces in between characters. Use lowercase for all fonts. 28b) In blank #2, type in your answer for the time it will take for 20% f the reactant to decompose. The answer is in seconds but do not include the unit. Enter your answer as a whole number with four significant figures.arrow_forward
- Sketch a potential energy diagram for the decomposition of nitrous oxide. N2O(g) →→ N2(g) + O(g) The activation energy for the forward reaction is 171 kJ; If the activation energy for the reverse reaction is 99 kJ, calculate the standard enthalpy change for this reaction. Transfer all the information into an energy diagram. label appropriatelyarrow_forwardQuestion 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1arrow_forwardWrite the reaction rate expressions for the reaction below in terms of the disappearance of the reactants and the appearance of products. Give the expressions for the disappearance of the reactants first, in the order written in the chemical equation. Then write the expressions for the appearance of the products in the order written in the chemical equation. Write the expressions in order of appearance in the equation in the form: ± 1 A[A] X At 2H₂(g) + O₂(g) Rate of H₂ = of O₂ = Rate of Rate of H₂O = X X X where ± is either a plus OR a minus sign, not both, X is an integer, and A is a chemical species. Do not include the state of matter. 2 H₂O(g) A[H₂] At 4[%₂] At 4[H₂O] At 00 X 3arrow_forward
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