Assuming atmospheric [Ar(g)] is 0.924 % (v/v) at 25°C and 1 atm, calculate the equilibrium [Ar(aq)] in freshwater (i.e., assume infinitely dilute)
Assuming atmospheric [Ar(g)] is 0.924 % (v/v) at 25°C and 1 atm, calculate the equilibrium [Ar(aq)]...
Use the data in the table below to calculate the equilibrium constant at 25°C for the reaction: Cl2(g) + Sn(aq) + Sn2+ (aq) + 2C1- (aq) Standard Reduction Potentials at 25°C Sn(aq) + 2e + Sn2+ (aq) E° = -0.14 V Cl2 (g) + 2e + 2C1- (aq) E° = 1.36 V Express your answer to two significant figures. O ALQ O a ?
Assuming that the atmospheric pressure at sea level is 1 atm, what is the pressure at a height of 500 m? Assume that at both levels the temperature is the same and equal to 300 K. 0.23 atm 0.06 atm 0.78 atm 0.94 atm
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.628 M , [Co2+]= 1.40×10−2 M , and [Cl−]= 0.652 M , and the pressure of Cl2 is PCl2= 7.80 atm ? Express your answer with the appropriate units. - Part A For the reaction 2CO3+ (aq) + 2CT (aq)+2Co2+ (aq) + Cl2(g). E=0.483 V what is the cell potential at 25°C if the concentrations are Co3+1 = 0.628 M, Co2+1...
12. At standard conditions (1M, 1 atm), the following reaction is spontaneous at 25°C. 40H (aq) +212 (1) ► 41- (aq) + O2(g) + 2H20 ( (balanced) If the pH is adjusted to 10.00, what will be the value of Ecell, and will this reaction be spontaneous? O2 (g) + 2H20 (1) + 4e → 12 (1) + 2e → 21 (aq) 40H (aq) E° = 0.40 V E° = 0.53 V
problem #9 Calculate the equilibrium constant for the following reaction at 25°C. 2H2(g) + O2(g) 2H20cv) Given the following standard free-energy: H2O , -237.2 KJ/mol at 25°C. Problem #10. Given the following data at 25°C: substance sº (J/mol.K) AH', (KJ/mol) 240.45, 33.8 304.33 9.66 NO 249) N2O160) (a) Calculate the value of A Gº for the following reaction at 25°C: 2 NO2(9) N20 (9) (b) Is the formation of NO a spontaneous process at 25°C and standard-state conditions? (a) What...
The vapor pressure of water at 25 degree C is o.0313 atm. Calculate the values of K_p and K_c at 25 degree C for the equilibrium: H_2O (l) H_2O(g). Vinegar contains acetic acid, a weak acid that is partially dissociated in aqueous solution: CH_3COOH(aq) H^+(aq) + CH_3CO^-_2 (aq) a) Write the equilibrium constant expression for K_c. b) What is the value of K_c if the extent of dissociation of 1.0 M CH_3COOH is 0.42%? Determination of an Equilibrium Constant
Calculate the (equilibrium) sublimation temperature of CO_2 at a pressure of 2 atm assuming a constant enthalpy of sublimation of Delta H-26 kJ/mol. he sublimation temperature of CO_2 at 1 atm is -78.5 degree C. Gold has an equilibrium melting temperature of 1337 K at 1 atm and an enthalpy of fusion of 12, 550 J/mol. Find the pressure at which the equilibrium melting temperature is 1400 K. The densities of solid gold and liquid gold are 19.3 g/mL and...
Atmospheric CO2 (g) is in equilibrium with dissolved CO, (aq), CO2(g) CO2 (aq) CO: (aq) then can react with water to become H_CO. CO2 (aq) + H:0 (1) ~ HCO, (aq) (2) Add the two reactions together and determine the overall net reaction. If the K, for reaction (1) is 1.44 x 10-4 and for reaction (2) the K is 1.90 x 10-2, then what would the K, for the overall net reaction be? Explain. Increasing CO, (g) would have...
For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.614 M , [Co2+]= 0.508 M , and [Cl−]= 0.321 M , and the pressure of Cl2 is PCl2= 7.90 atm ?