4.(4 points) What is the value of equilibrium constant for the system shown below at 25°C...
calculate the value of the equilibrium constant at 25 Celcius, for the reaction: HNO2 + OH- -> H2O + NO2- H3O+ and NO2-= 4.67 x 10^-3 M Ka of HNO2= 7.2 x 10^-4 M
The equilibrium constant for a reaction is 0.48 at 25 c. What is the value of AG (k/mol) at this temperature Seleccione una: a. 4.2 b. 1.8 d. 150 e. More information is needed. The equilibrium constant for a reaction is 0.48 at 25 cl What is the value of AG /mob at this temperature Seleccione una: a. 4.2 b. 18 c. 4.2 d. 150 e. More information is needed.
The equilibrium constant for a reaction is 0.35 at 25 °C. What is the value of AG* (kj/mol) at this temperature? A. 2.6 B.-4.2 C. 220 D.4.2 E. More information is needed.
For the following equation: The Ka value of HNO2 is 4.0 x 10-4. If the equilibrium concentration of HNO2 is 0.54 M. what is the equilibrium concentration of NO2/H30? 2 points HNO, + H, O NO + H20+ Your answer
The value of Ka for nitrous acid (HNO2) at 25 ∘C is
4.5×10−4.
Part D What is the value of AG when [H+] = 5.8 x 10-2M, [NOą] =6.4 x 10-4 M and (HNO2] = 0.21 M ? Express your answer using three significant figure. IVO AED A o 2 ? AG = Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Recall that AG = AGº + RTinQ, where R is the gas constant, T is...
Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium constant for the reaction shown at 800.0°C COCI, (g) 2 CO (g) + Cl2 (g) AG° = 69.46 kJ AH° = 110.38 kJ AS° = 137.24 J/K at 800.0°C
The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to reference(Pages 833 - 836) Section19.7 while completing this problem. Part A Write the chemical equation for the equilibrium that corresponds to Ka. Write the chemical equation for the equilibrium that corresponds to . H+(aq)+NO2−(aq)⇌HNO2(aq) HNO2(aq)⇌H+(aq)+NO2−(aq) HNO2(aq)⇌H−(aq)+NO2+(aq) HNO2(aq)+H+(aq)⇌H2NO2+(aq) HNO2(aq)+H−(aq)⇌H2NO2+(aq) Part B Using the value of Ka, calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. Express your answer using three significant figures. ΔG∘...
. Predict the direction in which the equilibrium will lie for the reaction NO2- (aq) + HClO3(aq) <----> HNO2(aq) + ClO3- (aq) Ka(HNO2) = 4 X 10-4 A) reactants will be favored B) products will be favored C) cannot be determined D) reactants and products will be equally favored E) depends on Kb values which are not given.
1. Consider reaction (1) shown below with it's associated equilibrium constant. What is the equilibrium constant for reaction (2)? Report your answer to THREE significant figures. (1) A + 3 B ⇌ 2 C , K = 0.259 (2) 2 A + 6 B ⇌ 4 C , K = ?? 2. The pressure-based equilibrium constant for the reaction shown below is KP = 3.575 at 443 °C. What is the value of KC at this temperature? 2 NO(g) + O2(g) ⇌...
4. A reaction has an equ reaction at this temperature. (25 points) has an equilibrium constant of K -0.018 at 25°C . Find AG run for the