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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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1. How many moles are contained in 34.0 grams of propane, C3H8, the gas used as a fuel for many barbecues?
2. Identify what would increase the rate of the following reaction:
2SO2(g) + O2(g) → 2SO3(g)
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- Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.36M 2.01 M 0.639 M/s 1.36M 4.86M 3.74 M/s 0.400M 2.01 M 0.188 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k -0 - x10 Śarrow_forwardGiven the following reaction, when [E] is decreasing at 0.2 mol/L s, how fast is [G] increasing? 2D(g) + 3E(g) + 5F(g) --> 7G(g) + 6H(g)arrow_forward10. Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO2(g) [NO] (M) [02] (M) Initial Rate (Ms ¹) A. Rate 57 M¹s¹ [NO][O₂] B. Rate = 3.8 M-1/2 5-1[NO][O₂] 1/2 C. Rate = 3.1 × 105 M¯³s¯¹[NO]²[O₂]² D. Rate = 1.7 × 10³ M²s¯¹[NO]²[02] E. Rate = 9.4 × 10³ M²s¯¹[NO][O₂]² -2 0.030 0.0055 8.55 x 10-3 0.030 0.0110 1.71 × 10°² -2 0.060 0.0055 3.42 × 10-2arrow_forward
- Help me please ASAParrow_forwardConsider the gas phase reaction between H2 and CO: H2O(g) + CO(g) --> CO2(g) + H2(g) When 4 moles of CO gas are reacting every 100 seconds in a 1L vessel, what is the rate at which H2 is produced?arrow_forwardRefer to the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g). If the reaction is second order with respect to both NO2 and CO, what happens to the reaction rate when the concentration of both reactants is doubled? O Reaction rate is also doubled O Reaction rate increases by a factor of 8 O Reaction rate increases by a factor of 16 Reaction rate increases by a factor of 32arrow_forward
- Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 2.48M 1.13M 84.0 M/s 0.635M 1.13M 2.48M 0.211 M rate = k [] 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 2 significant digits. Also be sure your answer has the correct unit symbol. k = 5.51 M/s 0 2.93 M/s x10 ■• X Śarrow_forwardFor the following reaction, the rate that the H2 is being consumed is 6.2 x 10-3 M/s. N2 (g) + 3 H2(g) --> 2NH3(g)Determine the rate of formation of (NH3) for this reaction at the same time. Select one: a. 4.1 x 10-3 M/s b. - 4.1 x 10-3 M/s c. 9.3 x 10-3 M/s d. -9.3x 10-3 M/s e. 1.3 x 10-2 M/sarrow_forwardthe question is on the imagearrow_forward
- #8arrow_forward7. Reactions A and B were studied and found to produce the given energy diagrams. 150 150 Energy 100 (kJ/mol) 100 Energy (kJ/mol) 50 50 Reaction progress Reaction progress Reaction A Reaction B A third reaction, C was studied with a measured activation energy of 55 KJ/mol. Assume all reactions take place at the same temperature. Reaction A is slowest a. b. Reaction B is slowest c. Reaction C is slowest d. All reactions happen at the same rate.arrow_forward1a Explain using an example how the rate of reaction is related to the rate of change of reactant or product concentration.arrow_forward
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