Please EXPLAIN and solve EACH/ALL part(s) in Question #10!

DOUBLE CHECK YOUR WORK AND ANSWER(S).

PLEASE NEATLY SHOW ALL WORK, EXPLANATIONS, & CALCULATIONS STEP-BY-STEP USING PEN AND PAPER! I AM NEW TO CHEMISTRY! I AM A COMPLETE NEWBIE!

Part 2 - Writing Equilibrium Expressions To clarify, the concentrations of reactants and products are not equal at equilibrium - rather, the rates of the forward and reverse reactions are equal. So what about the concentrations? What can we know about them? The concentrations become constant; they don't change once equilibrium is reached (as long as the temperature remains constant and no other stresses are placed on the system). We quantify the relative concentrations of reactants and products at equilibrium with a quantity called the equilibrium constant (K). Consider an equation for a generic chemical reaction: aA+bBcC+dD where A and B are reactants, C and D are products, and a,b,c, and d are the respective stoichiometric coefficients in the chemical equation. The equilibrium constant (K) for the reaction is defined as the ratio-at equilibrium-of the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients. In this notation, [A] represents the molar concentration of A. Why is this particular ratio of concentrations at equilibrium-and not some other ratio-defined as the equilibrium constant? Because this particular ratio is always a constant when the reactants and products are at equilibrium (at constant temperature). As we can see from the expression, the equilibrium constant quantifies the relative concentrations of reactants and products at equilibrium. The relationship between the balanced chemical equation and the expression of the equilibrium constant is the law of mass action. Now it's time to practice writing equilibrium expressions for gaseous and aqueous reactions. Part 4 - The Reaction Quotient, Q We use the reaction quotient, Q, to answer two specific questions: 1) Is a reaction system that contains both reactants and products at equilibrium? 2) Which direction will a system not at equilibrium proceed (will it shift left to form more reactants, or shift right to form more products)? The reaction quotient is calculated using the same formula as the equilibrium expression, but with the assumption that the system is not at equilibrium. QK Reaction goes to the left (toward reactants). Q=K Reaction is at equilibrium. Part 5-Reversing Chemical Reactions 10A. The equilibrium constant Kc for the equation 2HI(g)H2(g)+I2(g) at 425C is 1.84. What is the value of Kc for the following equation under the same conditions? H2(g)+I2(g)2HI(g) Insert an image of your work here. 10B. Consider the following chemical equation and equilibrium constant at 25C : 2COF2(g)CO2(g)+CF4(g)K=2.2106 Calculate the equilibrium constant for the following reaction at 25C : 2CO2(g)+2CF4(g)4COF2(g)K=? Insert an image of your work here