1.The equilibrium constant of a reversible process at 386 K is 9.2, what is the standard...

1.The equilibrium constant of a reversible process at 386 K is 9.2, what is the standard change in free energy for that process?

2. What is the reaction order for a process whose rate constant has units of M^-3 s^-1?

3. The standard molar entropy of solid iron at 298 K is 27.2 J/mol.K. How many microstates are associated with 50 atoms of iron at this temperature?

5. What is the pH of the solution that is formed when 10.0 grams of magnesium hydroxide is dissolved in 100.0 mL of water?

6. At 50ᵒC, Kw is 5.476 x 10^-14. What is the pH of pure water at that temperature?

7. A saturated solution of sodium sulfate can have 0.0979 mol of the salt dissolved in 100 mL of water. What is the Ksp of sodium sulfate?

8. The half-life of ²⁴¹Pu is 14.4 years. What percent of ²⁴¹Pu will be present 31 years later?

9. What is the boiling point of a 0.500 m aqueous solution of ammonium nitrate?

Expert Solution

TThe above questions have been solved using the required and existing formulas.

queen_honey_blossom answered 2 years ago

Determination of an Equilibrium Constant 1. What is meant by a reversible reaction? 2. True...

Determination of an Equilibrium Constant 1. What is meant by a reversible reaction? 2. True or False : The numerical value of the equilibrium constant for a given reaction only changes if the temperature changes. 3. Which component of the reaction mixture was it that was titrated with sodium hydroxide? A. Acetic acid B. Isopropyl alcohol C. Water D. ...

K CONSTANT EQUILIBRIUM What does it mean when K=1 and when K= 0

An elementary reaction A to B is reversible and has an equilibrium constant of 10, and...

An elementary reaction A to B is reversible and has an equilibrium constant of 10, and a forward rate constant of 1.0 d-1. a) Plot the concentrations of A and B as a function of time in a batch reactor that initially contains 10-3 M each of A and B. Show the data from the initial condition until the concentrations are both changing at an instantaneous rate of less than 10-5 M per day. b) Repeat part (a) if the...

Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K...

Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K of the reaction Cl2(g)+2NO(g)⇌2NOCl(g) The standard Gibbs energy change of the reaction represents the drive the reaction has under standard conditions to move toward equilibrium from point A to point X in the diagram. Substance ΔfG∘ (kJ mol−1) Cl2(g) 0 NO(g) 86.71 NOCl(g) 66.30

1)The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) The equilibrium...

1)The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <------ ------> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.14 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2) The equilibrium constant, Kp, for the following reaction is 55.6 at 698...

The equilibrium constant for the reaction below is K = 0.36 at 400 K. If 1.5...

The equilibrium constant for the reaction below is K = 0.36 at 400 K. If 1.5 g of PCl5 was initially placed in a reaction vessel with a volume of 250 cm3, what is the molar concentration of each gas at equilibrium? What is Delta Gorxn for the reaction: PCl5 (g) à PCl3 (g) + Cl2 (g) - Please show all work.

Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s)...

Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s) + Y^2+(aq) ⇌ X^2+(aq) + Y(s) K= 1.43 x 10^-6 E^o = ? V

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K...

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species. to the right to the left [N2] =____ mol/L [O2] = ____mol/L [NO]...

1) The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) <---...

1) The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) <--- ---> CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.206 M COCl2, 5.16×10-2 M CO and 5.16×10-2M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 2.88×10-2 mol of CO(g) is added to the flask? [COCl2] = M [CO] = M [Cl2] = M 2) The equilibrium constant,...

1) The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) <-----...

1) The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) <----- ------> PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.201 M PCl5, 4.91×10-2 M PCl3 and 4.91×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.27×10-2 mol of Cl2(g) is added to the flask? [PCl5] = M [PCl3] = M [Cl2] = M 2)...

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