1. At 1500K, the equilibrium constant for the reaction N 2 (g) + O 2 (g) ® 2NO(g

Question

1. At 1500K, the equilibrium constant for the reaction

N2 (g) + O2(g) ® 2NO(g)

has a value of 1.0x10-5. Calculate the concentration of N2 at equilibrium if initially 0.25 mol of NO is placed in a 1.0L container.

The answer is [N2] = 0.1248mol/l

2. Calculate the pH of a solution prepared by adding 5 mL of 0.5 M NaOH to 50 mL of 0.1 M iodoacetic acid (Ka = 6.68 x 10-4)

The answer is pH=3.18

3. Calculate the solubility of AgI in a solution, which contains 0.055 M calcium iodide.

The answer is 7.5x10-16

51. . Calculate the voltage of the following reaction

3I2(s) + 5 Cr2O72- + 34H+ ® 6IO3- + 10 Cr3+ + 17 H2O

if [Cr2O72- ] = 0.10 M, [H+ ] = 0.01, [IO3- ]=0.001 M and [Cr3+] = 0.0001 M

The answer is 0.105V

could you please explain the steps in details?

Explanation / Answer

K= 1*10-5 = 0.25*0.25/x2

x= 0.1248 M

2)

0.005*0.5 -0.05*0.1 = 2.5*10-3 moles of iodoacetic acid

Ka= 6.68*10-4 = x2/ 2.5*10-3

x= 1.29*10-3

pH = 3.18

3)

x= 4.125*10-17 /0.055

= 7.5*10-16

4)

3I2(s) + 5 Cr2O72- + 34H+  ®Ã‚    6IO3- + 10 Cr3+ + 17 H2O

if [Cr2O72- ] = 0.10 M, [H+ ] = 0.01, [IO3- ]=0.001 M and [Cr3+] = 0.0001 M

E= -0.0592/15* log(0.0001*0.001/0.1*0.01)

= 0.105V

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.