er is incorrect. wing equilibrium system: e, the rate of N-0 ale) being consumed is 1.0 M/s while the rate of NO e) being formed is 1.0 M m? ce of the forward reaction is equal to the rate of the reverse reaction. eof the forward reaction is greater than the rate of the reverse reaction. e of the forward reaction is less than the rate of the reverse reaction. ation provided is not sufficient to determine equilibrium position. Attempts: 2 of 3 used

er is incorrect. wing equilibrium system: e, the rate of N-0 ale) being consumed is 1.0 M/s while the rate of NO e) being formed is 1.0 M m? ce of the forward reaction is equal to the rate of the reverse reaction. eof the forward reaction is greater than the rate of the reverse reaction. e of the forward reaction is less than the rate of the reverse reaction. ation provided is not sufficient to determine equilibrium position. Attempts: 2 of 3 used

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 120QRT

See similar textbooks

Similar questions

Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.
Data in the table were collected at 540 K for the following reaction: CO(g) + NO2(g) CO2(g) + NO(g) Using the data in the table: (a) Determine the reaction order with respect to each reactant. (b) Derive the rate equation. (c) Calculate the rate constant, giving the correct units for k.
Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s)2NH3(g)+CO(g)+H2O(g) is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?
Dinitrogen trioxide decomposes to NO and NO2, in an endothermic process (rH = 40.5 kJ/mol-rxn). N2O3(g) NO(g) + NO2(g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more N2O3(g) (b) adding more NO2(g) (c) increasing the volume of the reaction flask (d) lowering the temperature
For the endothermic reaction AB(g)A(g)+B(g), the following represents a reaction container at two different temperatures. Which one (I or II) is at the lower temperature?
The following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an equilibrium among CH4, O2, CO2, and H2O established under these conditions? Explain your answer.
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH3CO2HAceticacid+C2H5OHEthanolCH3CO2C2H5Ethylacetate+H2OK=2.2 For the following mixtures (a-d), will the concentration of H2O increase, decrease, or remain the same as equilibrium is established? a. [CH3CO2C2H5] = 0.22M, [H2O] = 0.10M, [CH3CO2H] = 0.010 M, [C2H5OH] = 0.010 M b. [CH3CO2C2H5] = 0.22 M, [H2O] = 0.0020 M, [CH3CO2H] = 0.0020 M, [C2H5OH] = 0.10 M c. [CH3CO2C2H5] = 0.88 M, [H2O] = 0.12 M, [CH3CO2H) = 0.044 M, [C2H5OH] = 6.0 M d. [CH3CO2C2H5] = 4.4 M, [H2O] = 4.4 M, [CH3CO2H] = 0.88 M, [C2H5OH] = 10.0 M e. What must the concentration of water be for a mixture with [CH3CO2C2H5] = 2.0M, [CH3CO2H] = 0.l0 M, and [C2H5OH] = 5.0 M to be at equilibrium? f. Why is water included in the equilibrium expression for this reaction?
Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + |o2(g)^SO}(g) A, £ 2 SO,(g) «=* 2 SO,(g) + O,(g) A, Which of the following expressions relates A, to A2? A2 = A,2 A,2 = A, A2 = A, A2 = 1/A, A2 = 1/A,2
a Predict the direction of reaction when chlorine gas is added to an equilibrium mixture of PCl3, PCl5 and Cl2. The reaction is PCl3(g)+Cl2(g)PCl5(g) b What is the direction of reaction when chlorine gas is removed from an equilibrium mixture of these gases?
Consider the reaction A+BC+D. A friend asks the following: “I know we have been told that if a mixture of A, B, C. and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?” What do you tell your friend?