QUESTION 18.1 POINT The initial concentrations of Na+ and Cl” in the reaction below are each...
The initial concentrations of L, and I in the reaction below are each 0.0401 M. If the initial concentration of I, is 0.0 M and the equilibrium constant is K. 0.25 under certain conditions, what is the equilibrium concentration (in molarity) of 12 I, (aq) = L(aq) +T" (aq) • Your answer should include two significant figures.
Consider the reaction below. The initial concentration of KBr is 0.0183 M, and the initial concentrations of K+ and Br− are each 0 M. If the equilibrium constant is Kc=7.76 under certain conditions, what is the equilibrium concentration of KBr? KBr(aq)⇌K+(aq)+Br−(aq) Remember to use correct significant figures in your answer (round your answer to the nearest hundredth).
NaCl(s) ⇌ Na+(aq) + Cl-(aq) ΔHo = 3.9 kJ/mol At 298 K, a saturated solution of NaCl has [Na+] = 7.0 M and [Cl-] = 5.4 M. If the temperature of the mixture is increased to 323 K, what will be the equilibrium concentration (M) of Na+? (Assume no ion pairing.) Enter your answer to 2 decimal places. NaCl(s) Na (aq) + CI'(aq) AH- 3.9 kJ/mol At 298 K, a saturated solution of NaCI has [Na"] 7.0M and [CI] -...
14. What are the final concentrations of A and A, at equilibrium if the initial (A) concentration is 0.60M? K-4.2 x 10* As (g) 2A(8) Initial: 0.60 Equilibrium: 15. Find final equilibrium concentrations for HA, H', and A: HA(aq) + H20 (1) HO" (aq) + A' (aq) Initial Concentrations 0.60 M OM ом K.-2.0 x 10 **Remember to review Properties of liquids (solubility, intermolecular forces, colligative properties, concentration units), phase diagrams, phase changes and the energy associated with heating and...
Calculate the equilibrium concentrations of H2O, Cl, HCl, and O2 at 298 K if the initial concentrations are (H2O) = 0.070 M and (Cl2] = 0.120 M. The equilibrium constant Kc for the reaction H2O(g) + Cl2(g) + 2HCl(g) + O2(g) is 8.96 x 10 -9 at 298 K
The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] = The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362 M, calculate the [Br] =
2. For the acid dissociation reaction below, the equilibrium concentrations are given as [H'] = 0.0060 M, [C2H302] =0.0060 M and the equilibrium constant, K is given as 1.8 x10-5. HC2H3O2 (aq) + (aq) + C2H:O2 (aq) a) Write the equilibrium constant expression for the reaction b) Calculate the concentration of HC2H302 at equilibrium
The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as follows: [H2] = 1.0 x 102 M. [Na] - 4.0 M, and (NH) - 1.0 x 10* M. N (8) + 3H,() 2NH3(e) 3. Consider the chemical reaction: N2 + 3H2 yields 2NH3. If the concentration of the reactant Hy was increased from 1.0 x 10-2M to 2.5 x 10-M, calculate the reaction quotient (C) and determine which way the chemical system would shift...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...