Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Suppose a 350. mL flask is charged under these conditions with 100. mmol of hydrogen iodide. After how much time is there only 50.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.arrow_forwardChlorine dioxide, CIO₂, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO3 and ClO₂ ions. 2 CIO₂(aq) + 2 OH(aq) → CIO3(aq) + ClO₂ (aq) + H₂O(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO₂ was determined. Use the data here to determine the order of the reaction for CIO₂ and OH, and the value of the rate constant. [CIO2]init [OH Jinit Initial Rate, mol/(Los) Exp. 1 0.030 Exp. 2 0.060 Exp. 3 0.030 Order for CIO₂: Order for OH": Rate constant = 0.030 0.030 0.060 0.0062 0.0248 0.0124arrow_forwardUnder certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0029 M·s : 2 NH3 (g) → N, (g)+ 3 H, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of ammonia. After how much time is there only 200. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. х10arrow_forward
- Consider the hypothetical reaction A +B+ 2C → 2D + 3E where the rate law is ΔΙΑ = k[A][B]? At Rate An experiment is carried out where [A]o = 1.0 x 10-² M, [B]o 6.0 M, 2 and [C, = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mol -1 S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 19.0 seconds. Concentration M d. Calculate the concentration of C after 19 seconds. Concentration = Marrow_forwardConsider the following balanced chemical equation: H2O2 (aq) + 3 l"(aq) + 2 H* (aq) → l3 (aq) + 2 H2O (1) In the first 32.7 seconds of the reaction, the concentration of H2O2 decreased from 1.5 M to 0.72 M. What is the average reaction rate over this time interval (in mol L-1 s-1)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:arrow_forwardAt a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.0263 s : 2HI (g) - H, (g)+I, (g) Suppose a vessel contains HI at a concentration of 0.130 M. Calculate the concentration of HI in the vessel 35.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. ) M x10arrow_forward
- Consider the hypothetical reaction А +В+ 2C 2D + ЗЕ where the rate law is ΔΙΑ : 서A][B]2 Rate At An experiment is carried out where [A], = 1.0 x 10-2 M, [B], 3.0 М, and [C, = 2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is = 3.8 x 10- M. a. Calculate the value of k for this reaction. -2 L? mol s 1 k = b. Calculate the half-life for this experiment. Half-life c. Calculate the concentration of A after 18.0 seconds. Concentration = M d. Calculate the concentration of C after 18 seconds. Concentration Marrow_forwardThe catalyzed decomposition of ethanol at 328°C has a rate constant of 4.00 x 105 L mol ¹s¹. A graph of the reciprocal of ethanol concentration versus time gives a straight line. The chemical equation for the reaction at this temperature is C₂H₂OH() C₂H.(g) + H₂O(g) If the initial concentration of ethanol is 0.022 mol L¹, how long will it take for the pressure to reach 1.4 atm at 328°C? hoursarrow_forwardConsider this reaction: H,CO, (ag) – H,0 (aq) + CO, (ag) At a certain temperature it obeys this rate law. rate = (9.70 x 10-4s)H,co,] Suppose a vessel contains H,CO, at a concentration of 0.470 M. Calculate the concentration of H,CO, in the vessel 680. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10arrow_forward
- Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's : 2 NH, (g) → N2 (g) +3 H, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ararrow_forwardConsider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.arrow_forwardAt a certain temperature the rate of this reaction is second order in NH, with a rate constant of 0.191 M 2NH, (g) → N₂(g) + 3H₂(g) Suppose a vessel contains NH, at a concentration of 1.11 M. Calculate how long it takes for the concentration of NH, to decrease by 76.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. OP X G aarrow_forward
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