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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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At a certain concentration of reactants the rate of appearance of water in the following reaction is 0.32 M/s. HINT: Watch the sign of the rate!
4NH3 + 7O2 4NO2 + 6H2O
(A) What is the
(B) What is the rate of reaction of NH3? __________M/s
(C) What is the rate of reaction of NO2? _____________M/s
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- Reaction Molecularity Rate expression (a) HO + NO2 + ArHNO3 + Ar _________ (unimolecular, bimolecularter, molecular) rate =___ (b) H + Br2HBr + Br _________ (unimolecular, bimolecularter, molecular) rate =___ (c) CH3CHOCH3 + CHO _________ (unimolecular, bimolecularter, molecular) rate =___ Submit Answerarrow_forwardCurrent Attempt in Progress The reaction 2A + 2B M+Nhas the rate law: Rate = k[A]?. At 25°C, k = 0.0376 L mol1s1. If the initial concentrations of A and B are 0.387 M and O.459 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 68.7 seconds Hint Your answer is incorrect. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = i ! M [B] = i M Hintarrow_forward4) Consider the following reaction: Na2CO3 + HNO3 = CO2 + H2O + Na₂NO₂ When the concentration of HNO3 was tripled (3x), the overall reaction rate increased by the magnitude of 9. Wat is the reaction order with the respect to HNO3 ? 4 pts CHANGE THIS QUESTIONarrow_forward
- ::)/(/((//arrow_forward4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.arrow_forwardREACTION A +B + C Products [B](M) 1.0 2.0 1.0 1.0 Rate(M/s) 1.0E-4 4.0E-4 2.0E-4 2.0E-4 Trial 1 [A](M) [C](M) 1.0 0.010 1.0 0.010 3 1.0 0.020 2.0 0.010 Using the data in the table and the rate law below, identify the reaction order with respect to each reatant. Rate = k[A]M[B]^[c]P (Rate = k times [A] to the mth power times [B] to the nth power times [C] to the pth power) %3Darrow_forward
- Be sure to answer all parts. For the following general reaction, rate = k[A]2 and k=1.3 × 10 2 M¹g¹; A+B 2C Use this information to fill in the missing table entries. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 × 10-6 2 0.026 0.250 3 0.500 2.20 × 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: Marrow_forward6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction orderarrow_forwardEnabled: Exam 2 Be sure to answer all parts. Consider the reaction A+B Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A] (M) | [B] (M) Rate (M/s) A. 匚 1.50 1.50 2.50 01 x 07 Reaction 1.50 6.40 x 10 Proctorio is sharing your screen. Stop sharing < Prev 10 of 17arrow_forward
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