A chemistry graduate student is studying the rate of this reaction: - H2CO3(aq) H₂O (aq) + CO2 (aq) He fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds:

the numbers 1-3 are just sub questions, thank u!!

In Problem 4A, you are given initial concentrations and asked which direction the reaction will go.  This involves formulating the reaction quotient, Q and comparing it to the equilibrium constant, K.  If Q is smaller than K, the reaction will go forward.  If it is greater than K, the reaction will go in reverse.  This is what I call the “easy” version of a Type 5 problem – determining the direction.    Problem 4B asks what the concentrations will be at equilibrium.  This is a harder problem and it involves setting up the ICE chart and solving it.  I refer to this as the “hard” version of a Type 5 problem – determining not just the direction but what the concentrations are at equilibrium.  You will have to come back to this part of the problem when we have covered how to solve it.   4A)  Suppose you place some solid NH4HS in a flask containing 0.50 atm NH3 (g).  Which way will the reaction go?  (Given:  Kp = 0.11.)   NH4HS (s)              H2S(g)     +     NH3 (g)…

Can you help me with this?

⦁    4.  Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.

In which of the following reactions will the pressure increase upon completion of the reaction at constant temperature? O a. C(s) + O2(g) CO2(g) Ob C2H6O(1) + 302(g) - 2CO2(g) + 3H2O(I) Oc Cl2(g) + 3Fz(g) – 2CIF3(g) Od 4NH3(g) + 502(g) - 4NO(g) + 6H2O(g) O e 2NO(g) + O2(g)- 2NO2(g)

Given that the equilibrium concentrations of [N₂] = 0.0010 M, [C₂H₂] = 0.066 M, and [HCN] = 6.8 × 10-4 M, find the value of the equilibrium constant expression for the reaction: N₂(g) + C₂H₂(g) ⇒ 2 HCN(g) 7.0 × 10-3 3.4 x 10-1 2.9 2.3 × 10-4 4300 Question 8 Select ALL of the correct answers for this question. For the following reaction, the addition of which of these reagents will suppress the equilibrium (shift to the left)? + NH3 + H2O = NH4 + HỌ All of the above NaCl KOH None of the above NaOH

2 Name: Maile Velazquez Date: Period: 6 H-02 Equilibrium Assignment Instructions: Write the Law of Mass Action for each of the following chemical equations and then calculate the indicated missing variable using the provided information while at equilibrium. Ex H2O + COH₂+ CO₂ 1H2O+ 1CO1H2 + 1CO₂ [H2]¹[CO2]¹ K₂ = Кс 4.73 [H,O][CO] [CO2] = [H2]¹ (4.73)(0.0322)(0.0510) [H2O] 0.0322 M [CO₂] = = 0.0135088 (0.575) [CO] 0.0510 M [H2]¹[CO2] [CO2] = 0.0135 M [H2] 0.575 M [H,O][CO] H₂+2 A₁₂+ B₂ → AB3 [AB3] 0.146 M [A₂] 1.50 M K = K₁ = [B2] 0.240 M

Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 (CH3)3 N(aq) + H₂O(l)— (CH3)3NH+ (aq) + OH-(aq) K 00

Which of the reactions that do not occur can be made to occur if an acid catalyst is added to the reaction mixture?