The table below shows the equilibrium % of product in a mixture of A, B andpressures and temperatures. Please note that A, B and C are all gasesPressure (bar)1101002005002070Consider the following possible reactionsReaction 1:Reaction 2:10060A+2B=>CA+B==> 2CTemperature3003035454750What is the correct answer?A. The values in the table represent Reaction 1B. The values in the table represent Reaction 2C. The values in the table represent Reaction 1D. The values in the table represent Reaction 27002025354045C at varic4000and this reaction is endothermicand this reaction is endothermicand this reaction is exothermicand this reaction is exothermic

To predict the reaction which belongs to the data given in the question and predict whether the…

The table below shows the equilibrium % of product in a mixture of A, B and pressures and temperatures. Please note that A, B and C are all gases Pressure (bar) 10 100 200 500 20 70 Consider the following possible reactions Reaction 1: Reaction 2: 100 60 Temperature 300 30 35 45 47 50 A+2B=>C A+B=> 2C 700 20 25 35 40 45 C at varic 4000

The table below shows the equilibrium % of product in a mixture of A, B and pressures and temperatures. Please note that A, B and C are all gases Pressure (bar) 10 100 200 500 20 70 Consider the following possible reactions Reaction 1: Reaction 2: 100 60 Temperature 300 30 35 45 47 50 A+2B=>C A+B=> 2C 700 20 25 35 40 45 C at varic 4000

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ

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Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
5.22. True or false: If for a gas-phase reaction, then all equilibrium partial pressures of reactants and products must equal . Explain your choice.
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Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
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