Equilibrium constant is the product of the concentration of products divided by the product of the concentration of reactant with each term raised to their coefficients as power. Solid and liquid are not represented in equilibrium constant Expression.
Hence, K = [CsOH]2[H 2]
Express the equilibrium constart for the following reaction. 2 Cs(s) + 2 H2O(1) = 2 CsOH(aq)...
Consider the following equilibrium reaction: CaCO3 (s) + CO2 (g) + H2O (l) ⇌ 2 HCO3- (aq) + Ca2+ (aq) Which of these species should be included in the equilibrium constant expression (K) for this reaction? Select all that apply A.) Ca2+ (aq) B.) CaCO3 (s) C.) H2O (l) D.) CO2 (g) E.) HCO3- (aq)
The reaction given below is an acid-base reaction. HC2H302(aq) + CsOH(aq) ® H2O(l) + CsC2H302(aq) Select one: O True O False
Write the name of the following compounds: 1. CrBr3 2. MnO2 3. P204 4. This question has multiple parts: 1. Write the balanced equilibrium reaction for nitrous acid reacting with water. 2. Write the equilibrium expression for this reaction. 3. Would you expect Ka to be greater than 1 or less than 1 for nitrous acid? Draw the Lewis structure of CSH2. C is the central atom. If 43 mg of Cs is added to excess water, what volume of...
Cesium metal reacts with water to form aqueous cesium hydroxide and hydrogen gas. Choose the balanced chemical equation for this reaction. O 2 Cs (s) + 2 H2002 CsOH(aq) + H2() O 4 Cs (s) + 2 H20014 CsOH (aq) + H2(g) OCs (s) + H00) CaOH(aq) + H/a) O 2 Cs (s) + H200) 2 CsOH (aq) + H2(g) Cs (8) + 2 H200 CHOH (na) + 2 H2()
The following reaction was carried out in a 3.75 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.50 mol of C, 12.7 mol of H2O, 4.00 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q? Enter the reaction quotient numerically. Q = Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.810 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00...
Express the equilibrium constant for the following reaction. 3 P4(s) + 15 O2(8) = 3 P4010(s) OK =([P4] [O2]15)/([P401013) O K =([P401015)/([P4] [02]) O K =([P401013)/([P_]*[02]15) OK=1/([O2]15) O K = [02]15
1. Solve for K under the following conditions with the following reaction: PbO (s) + 2H + (aq) ⇌ Pb2+ (aq) + 2H2O (l) PbO (s) = 8.67 g [H + ] = 3.43 M [Pb 2+ ] = 0.311 M H2O (l) = 5.02 M Find K 2. H2 (g) + I2 (s) ⇌ 2 HI (g) 0.162 atm H2 (g), 8.012 g I2 (s), 1.449 atm HI (g) Calculate the pressures of H2 and HI at equilibrium.
28. Use the standard reduction potenital to calculate equilibrium constants for the following reaction. H2O (1) H (aq) +OH (aq) at 298.15 K H2 (g)2H (aq) +2e 2H2O (aq) +2e - H2+ 20H (aq) A.K=1.0 x10 B. K=1.6 x10-1l C.K=1.0 x10-14 0 Define electrolvsis. E= 0V E -0.8277 V -10 spontaneous nonspontaneous nonspontaneous
Express the equilibrium constant for the following reaction. P4(s) + 5O2(g) ⇌ P4O10(aq) K =___ A. A) = [P4O10] / [P4] B. B) = [P4O10] / [P4][O2]5 C. C) = [P4O10] / [O2]5 D. D) [O2]-5 E. E) none of these
Determine the equilibrium-constant expression for the reaction: CuO(s) + H2(g) ⇌ Cu(l) + H2O(l) ? A. K = [H2O]/[CuO] B. K = [Cu][H2O]/[H2][CuO] C. K = 1/[H2] D. K = [H2]/[Cu]