Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Le Chatelier’s principle states that “If you stress a system at equilibrium, the system will react to relieve the stress and return to equilibrium”. The following equation represents a
2A (g) + 3B (g) <===> 2C (g) + 4D (g) ∆H = -378 kcal/mol (g) means gas
In each case below, explain how the system reacts (forward direction, reverse direction or no change):
- The concentration of A is increased
- Heat is added to the system
- B is removed from the reaction
- Pressure is added
- The concentration of C is increased
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- Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.arrow_forwardWhich is true of a system at equilibrium when Kc < 1? O Equilibrium favors neither reactants or products Equilibrium favors products O Equilibrium favors reactants Equilibrium is shifting to the left Equilibrium is shifting to the rightarrow_forwardThe equilibrium system between sulfur dioxide gas, oxygen gas, and sulfur trioxide gas is given. 2SO2(g)+O2(g)↽−−⇀ 2SO3(g)2SO2(g)+O2(g)↽−−⇀ 2SO3(g) Write the balanced chemical equation for the reverse reaction. Include physical states for all species.arrow_forward
- Consider the following reaction. 2 NO, (g) = N,04(g) When the system is at equilibrium, it contains NO, at a pressure of 0.872 atm, and N,O, at a pressure of 0.0760 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO, = atm PN,0, atmarrow_forwardCoal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gasarrow_forwardWrite the equilibrium 6H2O(g) + 6CO2(g) C6H12O6(s) + 6O2(g)arrow_forward
- Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) A catalyst is added to the reaction mixture. which will happen? the equilibrium will not shift the equilibrium will shift towards product but keq will not change the equilibrium will shift towards reactant but keq will not change the equilibrium will shift towards product and keq will increase the equilibrium will shift towards reactant and keq will decrease (b) The total pressure of the system is increased by adding a noble gas. (c) Cl2(g) is removed from the system.arrow_forwardA mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) ⥂ 2 SO3 (g) At equilibrium, 0.0916 mol of SO3 is present. a.) What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b.) If the container size is 3.0 L, what is the value of the equilibrium constant?arrow_forwardFor 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 reactantsarrow_forward
- For the reaction of nitrogen and oxygen to form nitrogen dioxide, N2(g) + 2 O2(g) → 2 NO2(g) Kc = 1.5×103 If the reaction mixture is found to contain 2.0 M NO2 and 0.10 M N2 and 0.10 M O2, what is the value of Q and what does this mean? is supposed to be an equilibrium arrow Q = 2x102 and the reaction will proceed towards the reactants. Q = 2x102 and the reaction will proceed towards the products. Q = 4x103 and the reaction will proceed towards the reactants. Q = 4x103 and the reaction will proceed towards the products.arrow_forwardConsider 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 H2arrow_forward
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