The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is approached?Othere will be a net gain in productthe reaction is at equilibriumO there will be no net gain in either product or reactant.there will be a net gain in reactantthere will be a net gain in both reactant and product

The reaction quotient (Q) for a system is 70. The equilibrium constant of system, Kc = 35

The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is approached? there will be a net gain in product the reaction is at equilibrium there will be no net gain in either product or reactant. there will be a net gain in reactant there will be a net gain in both reactant and product

The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is approached? there will be a net gain in product the reaction is at equilibrium there will be no net gain in either product or reactant. there will be a net gain in reactant there will be a net gain in both reactant and product

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

Ff.294.
When heat is added to exothermic reactions the equilibrium shifts towards the products. True False
11
Define equilibrium constant Keq
Consider the following system at equilibrium: CH4(g) + 2H20(g) CO2(g) + 4H2(g) What change will cause the equilibrium to shift to form more CH4? Multiple Choice decrease (H2] increase (H20] decrease the volume of the reaction vessel increase (CH4] decrease [CO2] DELL
Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the reactant concentrations drop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the product concentrations rise. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the forward rate constant drops.
c. HF & HCIO4 d. HBr & LIOH e. CH3COOH & KOH A sealed 1.00L flask is charged with 0.500 mol of I, and 0.500 mol of Br2. An equilibrium reaction ensues: 12 (g) + Br2 (g) =2 IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K is Select one: O a. K= 6.10 O b. K = 2.82 OC K = 882 Od. K= 110 Oe K= 131 en 13 The heat capacity of silver (Ag. 107.9 g maol), is 0.232 J g'K Calculate the energy needed to heat 2e mo saved II
For the equilibrium shown below, assess whether the following mixture is at equilibrium. If the mixture is NOT at equilibrium, tell whether the reaction will form more reactant or more products to reach equilibrium. 2 CO2 (g) 2 CO (g) + O2 (g) Kc = 6.4 x 10-7 [CO2] = 5.3 x 10-2 M [CO] = 3.6 x 10-4 M [O2] = 2.4 x 10-3 M
Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.
For the following reaction 2 SO2(g) + O2(g) <-> 2 SO3(g) + heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants
Use the following reaction to answer the questions below. N2 (9) + 3 H2 (g) → 2 NH3 (9) + heat Increasing the temperature of the reaction would cause the equilibrium to shift in which direction? Towards the products Towards the reactants No shift would occur Cannot be determined with the given information Increasing the amount of hydrogen in the reaction would cause the equilibrium to shift in which direction? Towards the products Towards the reactants No shift would occur Cannot be determined with the given information
Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2