∆G for the reaction AgBr(s) ⇌ Ag+(aq) + Br- (aq) is 69.9 kj/mol at 25C. What...

∆G for the reaction AgBr(s) ⇌ Ag+(aq) + Br- (aq) is 69.9 kj/mol at 25C. What is the molar solubility of AgBr(s) at this temperature?

Expert Solution

in this question, Gibbs free energy is given but at equilibria, it should be zero...so may be by mistake it has written ...so I corrected that question ... I have taken that as a standard Gibbs free energy and then I was able to calculate the solve the question... I hope this will help u ..thank u

queen_honey_blossom answered 2 years ago

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would...

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would be the value of K for AgBr(s) + 2NH3(aq) <--> Ag(NH3)2+(aq) + Br -(aq) ? b) What would be the molar solubility of silver bromide in 2.00 M aqueous ammonia?

at 25c the standard enthalpy of formation of HF(aq) is -320.1 kj/mol. of OH(aq) it is...

at 25c the standard enthalpy of formation of HF(aq) is -320.1 kj/mol. of OH(aq) it is -229.6Kj/mol. of F (aq) it is -329.2 Kj/mol.of H2O(l) it is -285.9Kj/mol. a. calculate the standard enthalpy of neutralization of HF. HF (aq) + OH- (aq) -->F-(aq) +H2O (l) b.using the value of -56.2kj as the standard enthalpy change for the reaction H+(aq)+ OH(aq)->H2O(l) c. calculate the standard enthalpy of change for the reaction HF->H+F

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.

You are given the equation: AgBr + 2S2O32- ---> Ag(S2O3)23- + Br - What mass of...

You are given the equation: AgBr + 2S2O32- ---> Ag(S2O3)23- + Br - What mass of AgBr can be dissolved by 750 mL of 0.300 M Na2S2O3? I know that the answer is 21.1 g AgBr, but I am not sure how you get to this point. (What are the steps to get this answer?)

For the following acid-base reaction H₂S(aq) + CN⁻(aq) ⇌ HS⁻(aq) + HCN(aq) ∆H° = -24.7 kJ/mol...

For the following acid-base reaction H₂S(aq) + CN⁻(aq) ⇌ HS⁻(aq) + HCN(aq) ∆H° = -24.7 kJ/mol and ∆S° = -49.9 J/mol･K. If you mix 100 mL of 0.0150 M NaCN with 100 mL of 0.0150 M H₂S, after equilibrium is established at 25°C what will be the molar concentration of HCN?

balance the following redox reaction in basic solution Ag(s)+CN-(aq)+ O2(g) -->Ag (CN)2- (aq) cyanide is not...

balance the following redox reaction in basic solution Ag(s)+CN-(aq)+ O2(g) -->Ag (CN)2- (aq) cyanide is not participating in the electrochemical reaction but does associate with the silver ion formed in a second association reaction. Balance the electrochemistry first and then add in the cyanide in by adding an associative reaction to the redox reaction.

Reaction 1: Cu(s) + AgNO3 (aq) = CuNO3 (aq) + Ag (s) Reaction 2: Cu (s)...

Reaction 1: Cu(s) + AgNO3 (aq) = CuNO3 (aq) + Ag (s) Reaction 2: Cu (s) +AgNO3 (aq) = Cu(NO3)2 (aq) + Ag (s) Part 1: Write the balanced net ionic equations for both of the above reactions. Assume that excess silver nitrate is available when answering the remaining questions. Part 2: Calculate the theoretical grams of silver metal that could form from 2.568g of copper wire based upon reaction 1. (Be sure the reaction is properly balanced.) Part 3:...

Calculate the equilibrium constant K of the reaction Sn(s)|Sn2+(aq)||Ag+(aq)|Ag(s) at 25 °C.

For the reaction CuS(s) + H2(g) H2S(g) + Cu(s), G°(CuS) = –53.6 kJ/mol G°(H2S) = –33.6...

For the reaction CuS(s) + H2(g) H2S(g) + Cu(s), G°(CuS) = –53.6 kJ/mol G°(H2S) = –33.6 kJ/mol H°(CuS) = –53.1 kJ/mol H°(H2S) = –20.6 kJ/mol Calculate the value of the equilibrium constant (Kp) at 200°C and 1 atm pressure

Ca(s)+2H(aq)--> Ca^2+(aq)+H2 ∆H= -543 KJ/mol CaCO3(s)+2H(aq)-->Ca^2+(aq)+CO2(g)+H2O(l) ∆H= -15 KJ/mol Look up the heats formation for CO2...

Ca(s)+2H(aq)--> Ca^2+(aq)+H2 ∆H= -543 KJ/mol CaCO3(s)+2H(aq)-->Ca^2+(aq)+CO2(g)+H2O(l) ∆H= -15 KJ/mol Look up the heats formation for CO2 and H2O in the thermodynamic tables and use this information along with the above heats of reaction to calculate the standard enthalpy of formation for CaCO3. Write the balanced equations for the two heat of formations reactions, and use Hess Law in order to answer this question.

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