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Write the equilibrium constant for C(s) + 2H2(g) ↔ CH4(g)

The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq)  which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in Molarity at equilibrium?   1.97 x 10-2   2.78 x 10-2   2.38 x 10-2   1.74 x 10-2   3.24 x 10-2   2.99 x 10-2   2.57 x 10-2   2.11 x 10-2   1.55 x 10-2   1.35 x 10-2

The equilibrium constant expression for the reaction CuO(s) + H₂(g) = Cu(s) + H₂O(g) is Kc = [H₂]/[H₂O]. True or False

2 Zn*2 (aq) +Fe*2 (ag) + 6 CN (ag) = Zn2Fe(CN)6 (5) [znz Fe (CN),] A certain equilibrium reaction has K = 2.8 x 10-13 at 25 °C. What is the change in Gibbs Free Energy (kJ/mole) under these conditions?

Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH:NH2(aq) + HCIO:(aq)- |3- 2- 4- 2+ |3+ 4+ 1 2 3 4 5 6 7 8 O2 O3 D4 Os |1 6. 10 (s) (1) (g) (aq) + H2O H3O+ H CI OH- C Reset x H2O Delete

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCN (aq) + OH" (aq) CN" (aq) + H,0 (1) K =

Write an expression for the equilibrium constant  for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)

Consider the following reactions: CO (g) + 2 H2S (g) D CS2 (g) + H2O (g) + H2 (g)         K1 = 1.3 x 105 ½ CH4 (g) + H2S (g) D ½ CS2 (g) + 2 H2 (g)                 K2 = 180   1. Find the equilibrium constant for: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) 2. What molecules in the steps are reaction intermediates? 3. If 0.500 atm of CO, H2, CH4, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.

2:25 1 Question 17 of 25 Submit Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O, and 0.200 mol N20 and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N20(g) + 3 O2(g) =4 NO2(g) 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 N20(g) + 3 O2(g) = 4 NO2(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190 0.0410 0.0710 0.0360 0.180

Calculate Kc or Kp:CH4(g)+H2O(g)->CO(g)+3H2(g) Kp=7.7x10^24 (at 298 K)

Given: 2N2(g)+ O2(g) = 2N20(g); Ke(1) = 5.8 x 10-36 and N2(g) + O2(g) = 2NO(g); K(2) = 4.1 x 10-31 What is the equilibrium constant for the reaction? 2N20(g) + O2(g) = 4NO(g)

The equilibrium constant (K1) for the reaction CO2 (g) 2 CO(g)+1/2 O2(g) is 6.66 x 10-12 at 1000 K. Calculate K2 for the reaction CO(g) +1/2 0,(g) 2 CO2 (g) K2 = %3D

The reaction N2O4−⇀↽−2NO2 is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.327 mol/L N2O4 and 1.91 mol/L NO2 . Calculate the equilibrium constant, Kc , for this reaction. Kc= 11.16     An additional 1.00 mol NO2 is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. towards the product towards the reactant no change Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc . Kc will increase Kc will not change Kc will decrease Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N2O4]=   mol/L [NO2]=   mol/L

Consider the reaction: HCI(aq) + NH, (ag) – NH,Cl(aq) Where 20.00 mL of 0.100 M NH, (aq) is added to 10.00 mL of 0.200 M HCl(aq). Order the solution components (excluding water) from highest to lowest concentration. O [OH¯] > [NH3] > [Na*] > [Cl¯] > [H,O*] O (CI ] = [NH†] > [NH,] = [H,O*]> [OH¯] O [H,0*)> [Cl¯] > [NH,] > [NH†]> [OH) O [NH]= [OH"] > [H,O*] = [CI¯] > [NH,] O [H,0*] = [CI¯] > [NH,] > [NH ] = [OH] O [NH,CI] = [NH,] = [HCl] O [CI] > [NH†]> [H,O+] > [NH,] > [OH ] O INH,CI] > [NH3] > [HCl] O None of these

Use your knowledge about solubility rules and reactions to write (1) a balanced chemical  equation (molecular equation), (2) a total ionic equation, and (3) a net ionic equation for the  reactions below. Include the appropriate phase for each species. Do your experimental  observations match your predictions? (k) NaOH(aq) + SrCl2(aq) →

Copper(I) ions in aqueous solution react with NH3(aq) according toCu+(aq) + 2NH3(aq) → Cu(NH3)2+(aq) Kf = 6.3 × 1010Calculate the solubility (in g·L-1) of CuBr(s) (Ksp = 6.3 × 10-9) in 0.62 M NH3(aq).62.3solubility of CuBr(s):

Suppose the reaction system UO2 (s) + 4 HF (g) ↔ UF4 (g) + 2H2O (g) has already reached equilibrium.  Predict the effect that each of the following changes will have on the equilibrium position.  Tell whether the equilibrium will shift to the right, shift to the left, or will not be affected. Additional UO2 (s) is added to the system. The reaction is performed in a glass reaction vessel; HF (g) attacks and reacts with glass. Water vapor (H2O (g)) is removed.

Ff.136.