15- 2 NO(g) + O2(g) →2 NO2(g) For the reaction above, the rate constant at 380°C for the forward reaction is 2.6x103 liter/mole"-sec and this reaction is first order in O2 and second order in NO. The rate constant for the reverse reaction at 380°C is 4.1 liter/mole-sec and this reaction is second order in NO2. (a) Write the equilibrium expression for the reaction as indicated by the equation above and calculate the numerical value for the equilibrium constant at 380°C. (b) What is the rate of the production of NO2 at 380°C if the concentration of NO is 0.0060 mole/liter and the concentration of O2 is 0.29 mole/liter? (c) The system above is studied at another temperature. A 0.20 mole sample of NO2 is placed in a 5.0 liter container and allowed to come to equilibrium. When equilibrium is reached, 15% of the original NO2 has decomposed to NO and O2. Calculate the value for the equilibrium constant at the second temperature.

15- 2 NO(g) + O2(g) →2 NO2(g) For the reaction above, the rate constant at 380°C for the forward reaction is 2.6x103 liter/mole"-sec and this reaction is first order in O2 and second order in NO. The rate constant for the reverse reaction at 380°C is 4.1 liter/mole-sec and this reaction is second order in NO2. (a) Write the equilibrium expression for the reaction as indicated by the equation above and calculate the numerical value for the equilibrium constant at 380°C. (b) What is the rate of the production of NO2 at 380°C if the concentration of NO is 0.0060 mole/liter and the concentration of O2 is 0.29 mole/liter? (c) The system above is studied at another temperature. A 0.20 mole sample of NO2 is placed in a 5.0 liter container and allowed to come to equilibrium. When equilibrium is reached, 15% of the original NO2 has decomposed to NO and O2. Calculate the value for the equilibrium constant at the second temperature.

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

part c?
Choose the correct molecularity and rate law for each of the elementary reactions shown below. (a) Cl(g) + CCl3(g) CCl4(9) Molecularity: ---Select--- V (b) SO3(9) SO₂(g) + 0(g) Molecularity: ---Select--- (c) NO₂(g) + SO₂(g) NO(g) + SO3(9) Molecularity: ---Select--- (d) 2 NO₂(g) N₂04(9) Molecularity: ---Select--- (e) CH₂OOCH3(g) 2 CH₂O(g) Molecularity: ---Select--- Rate Law: Rate = k [CC14]² Rate = k [CI] [CC13] Rate = k [CI]² [CC13]² Rate = k [CCl4] Rate Law: Rate = k [S0₂] [0] Rate = k [SO3] Rate = k [SO3]² O Rate = k [S0₂]² [0]² Rate Law: O Rate = k [NO₂] [SO₂] Rate = k [NO₂]² [S0₂]² O Rate = k [NO]² [S03]² O Rate = k [NO] [S03] Rate Law: O Rate = k [NO ₂] Rate = k [N₂04]² Rate = k [N₂04] O Rate = k [NO₂]² Rate Law: O Rate = k [CH30] Rate = k [CH300CH3]² Rate = k [CH30]² Rate = k [CH3OOCH3]
Sort the following elementary reactions as unimolecular (1), bimolecular (2) or termolecular (3) and write down the rate law expression for that step Elementary step from reaction mechanism Molecularity Rate law for elementary step (CH3)3CBR → (CH3);C* + Br 2NO2 → N204 CH;CI +I → CH3I + Cl H* + Br - + H202 → HOB + H20 ONBR + ONBr → NO + NO + Brz N2O2 → NO + NO 03 > 02 + 0
The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(g) +SİH4(g)–→HI(g) +SIH3I(g) The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols. (a) Calculate the Arrhenius factor A for this reaction. L mols1 (b) Calculate the rate constant for this reaction at 235°C. L molls1
Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: Step 1: NO2 + NO2 NO + NO3 Step 2: NO3 + CO NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations. (b) Identify the intermediate(s). NO3 NO2 NO CO2 CO (c) Identify the rate-determining step. Step 1 Step 2 Neither step
13.74 Methyl acetate, CH,COOCH3, reacts in basic solu- tion to give acetate ion, CH;COO , and methanol, CH,OH. CH,COOCH,(ag) + OH (ag) → CH;COO (ag) + CH;OH(aq) The overall order of the reaction was determined by start- ing with methyl acetate and hydroxide ion at the same con- centrations, so [CH,COOCH3] = [OH]= x. Then Rate = k[CH,COOCH;"[OH¯]" = kx"*n %3D %3D Determine the overall order and the value of the rate con- stant by plotting the following data assuming first- and then second-order kinetics. Time (min) [CH,COOCH;] (mollL) 0.00 0.01000 3.00 0.00740 4.00 0.00683 5.00 0.00634 10.00 0.00463 20.00 0.00304 30.00 0.00224
1(a) A reaction is observed to have the following rate constants at the indicated temperatures. Assuming the frequency factor remains the same, estimate the activation energy of the reaction. T (in °C) 20 40 k (in per second) 45 576 O - 97000 J mol1 O ~97 J mol 1 O ~847 J mol1 O - 8.47 J mol·1 O ~847000 J mol1 1(b) The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP? O NO O NH3 O HE O Ne O CH4
For the first-order reaction N2O5( g) • 2 NO:(8) +0x8) t1/2 = 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1013 s-1, determine the value of k at 50°C. 3.
Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression (a) NO2 + NO2→2 NO + 02 rate = (b) BrONO- ЭBro + NOz rate = (c) 0+ 02 + M 03 + M rate = unimolecular bimolecular termolecular
Give written answer only
56. For the first-order reaction 2 NO₂(g) + O₂(g) N₂O5(g) t1/2 = 22.5 h at 20 °C and 1.5 h at 40 °C. -1 (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.05 × 10¹³ s-¹, determine the value of k at 30 °C.
For the first-order reaction N2O5( g) 2 NO2 g) + → t1/2= 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 105 s', determine the value of k at 50°C.