Question
Please Help me with this multiple choice questions, i would appreciate it
Reaction 1 has a Keq of 20.0020, reaction 2 has a Keq of 1.00 x 10-5, reaction 3 has a Ka of 0.32 and reaction 4 has a Kd of 2.1. Based on the equilibrium constants given, which of these reactions lies furthest towards products at equilibrium? reaction 1 b. reaction 2 c. reaction 3 d. reaction 4 e. when all reach equilibrium all will lie equally to the products side (that's what equilibrium means)The oxidation of an aldehyde using Cr2O7 makes the corresponding carboxylic acid and Cr2O3 in an aqueous equilibrium reaction. Cr2O7 is bright yellow and CrO3 is dark orange when in solution. If a more powerful oxidizing agent like OsO4 were added to this system which of the following would happen (assume the OsO4 itself doesn't contribute to the colour and don't worry about balancing the equation): the solution will become more yellow the solution will become more orange the solution will become more colourless there will be no change in colour e. none of the above will occur Which of the following is NOT or example of a heterogeneous equilibrium: salt dissolving in H2O ice melting in a closed container ammonia vapours coming off of smelling salts in a closed environment a weak aqueous acid dissociates in water lowering the pH of the solution all of these are hetergeneous equilibria
Explanation / Answer
1-a
2-b
3-e