Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g)  heat + 4NO(g) + 6H2O(g)                                b) heat + 2NaHCO3(s)   Na2CO3(s) + CO2(g) + H2O(g)

MOving to anotrie question will save this response. Question 7 A state of dynamic equilibrium, Ag2CO3(s) +→ 2Ag*(aq) + CO32(aqg), exists in solutida. Which direction will the equilibrium shift if Ca(NO3)2(aq) is added to the system? O To the left. O To the right. O It will not shift left or right. A Moving to another question will save this response. MacBook Pro 80 888 FS F6 F7 FA esc F2 %23 2$ 8. 2 3 4. Q K A D 5

What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s)   2 HI (g) + Cl2 (g)

Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.

Write the equilibrium 6H2O(g) + 6CO2(g) C6H12O6(s) + 6O2(g)

Consider the following reaction. 2 NO₂(g) = N₂O4(g) 4 When the system is at equilibrium, it contains NO₂ at a pressure of 0.860 atm, and N₂O at a pressure of 0.0740 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? atm PNO₂ = atm PN₂0₁ =

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 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. which will happen? 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 and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. 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 and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…

Hi! I am struggling with the synthetic route between these two. Would I brominate and then use an E2 base to create an alkene on the cyclohexane, and then do an organoboron with hydroxide and peroxide to create an alcohol and then covert the alcohol to tosylate?