Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. = (0.595 M²¹-s¯¹) [C₁₂05] rate = Suppose a vessel contains C1₂O5 at a concentration of 0.850 M. Calculate the concentration of C1₂O5 in the vessel 31.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10

Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. = (0.595 M²¹-s¯¹) [C₁₂05] rate = Suppose a vessel contains C1₂O5 at a concentration of 0.850 M. Calculate the concentration of C1₂O5 in the vessel 31.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate =(0.0913 s¯¹)[C₁₂05] Suppose a vessel contains Cl₂05 at a concentration of 0.460M. Calculate the concentration of C1₂O5 in the vessel 9.70 seconds later. You may assume no other reaction is important. 25 2 Round your answer to 2 significant digits. [ M x10
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
Consider this reaction: 2Cl,05 (g) → 2C1, (g) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.0272 Ms)[ci,037² -1 'S Suppose a vessel contains Cl,O, at a concentration of 0.300M. Calculate how long it takes for the concentration of Cl,O, to decrease to 20.0% of its initial 5. value. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10
3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
Consider this reaction: CICH, CH, CI (g) → CH,CHCI (g) +HC1 (g) At a certain temperature it obeys this rate law. rate = (0.0361 s")[CICH,CH,CI] Suppose a vessel contains CICH,CH,Cl at a concentration of 0.860M. Calculate the concentration of CICH,CH,Cl in the vessel 36.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
1a) A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt = k[A][B] The rate constant is 1.13×102 L mol-1 s-1 at 346.0°C and 3.55×103 L mol-1 s-1 at 548.0°C. Use the Arrhenius equation k = Ae-Ea/RT to: Calculate Ea for this reaction. 1b) Calculate the rate constant k at 416.0°C for this reaction. 1c) Calculate the pre-exponential factor A for this reaction.
Consider this reaction: NH₂OH(aq) →NH3(aq) + H₂O (aq) At a certain temperature it obeys this rate law. -1 -1 rate -(0.00284 M¹¹) [NH₂OH]² Suppose a vessel contains NH₂OH at a concentration of 1.33M. Calculate the concentration of NH₂Oн in the vessel 840. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
23. Consider the following reaction: 2 NO2(g) + O3(g) N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____ M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____ M/s