Question

In: Chemistry

Estimate the value of the equilibrium constant at 505 K for each of the following reactions....

Estimate the value of the equilibrium constant at 505 K for each of the following reactions.

2CO(g)+O2(g)⇌2CO2(g)

2H2S(g)⇌2H2(g)+S2(g)

Expert Solution

1.

2 CO(g) + O2(g) ----------------- 2 CO2(g)

G rxn = 2x Gf CO2 - [ 2xGf CO + Gf O2]

= 2x(-394.38) -[ 2x(-137.38 + 0.0]

= -788.76 +274.76

Grxn = -514 KJ

R = 8.314x10^-3 KJ , T = 505 K

Grxn = - RTlnK

Grxn = - 2.303 RTlogk

-514 = -2.303 x 8.314x10^-3 x 505 xlogk

logk = 514/9.669 = 53.16

K = 10^53.16

K= 1.44x10^53

2)

2 H2S(g) ---------------- 2H2(g) + S2(g)

Grxn = [2xGfH2 + G S2]- 2xGf H2S

= 2x0.0+80.08 - [2x(-33.05)]

= 80.88+66.1

= 146.18KJ

Grxn = 146.18KJ

Grxn = - RTlnK

Grxn = - 2.303 RTlogk

146.18 = - 2.303 x 8.314x10^-3x505 xlogk

logk = -146.18/9.669

logK= -15.11

K = 10^-15.11= 7.76x10^-16

K = 7.76x10^-16.

queen_honey_blossom answered 2 years ago

Estimate the value of the equilibrium constant at 675 K for each of the following reactions....

Estimate the value of the equilibrium constant at 675 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. 3 significant figures in answer. A. 2NO2(g)⇌N2O4(g) ΔH∘f for N2O4(g) is 9.16 kJ/mol. B. Br2(g)+Cl2(g)⇌2BrCl(g) ΔH∘f for BrCl(g) is 14.6 kJ/mol.

Estimate the value of the equilibrium constant at 640 K for each of the following reactions....

Estimate the value of the equilibrium constant at 640 K for each of the following reactions. ΔH∘f and S∘ for BrCl(g) is 14.6 kJ/mol and 240.0 Jmol⋅K, respectively. for the following 1. 2NO2(g)⇌N2O4(g) 2.Br2(g)+Cl2(g)⇌2BrCl(g)

Q.26 Estimate the value of the equilibrium constant at 620 K for each of the following...

Q.26 Estimate the value of the equilibrium constant at 620 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. Part A 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol. Express your answer using three significant figures. K = Part B Br2(g)+Cl2(g)⇌2BrCl(g) .ΔH∘f for BrCl(g) is 14.6 kJ/mol. Express your answer using three significant figures. K =

Use the standard reduction potentials to calculate the equilibrium constant for each of the following reactions:...

Use the standard reduction potentials to calculate the equilibrium constant for each of the following reactions: Note if deltaG° for each reaction would be greater than or less than zero. Co2+(aq) + Sn(s) = Co(s) + Sn2+(aq) Ag+(aq) + Cr2+(aq) = Ag(s) + Cr3+(aq)

1. The equilibrium constant is given for one of the reactions below. Determine the value of...

1. The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. 2 HD(g) ↔ H2(g) + D2(g) Kc = 0.28 3 H2(g) + 3 D2(g) ↔ 6 HD(g) Kc = ? 2. The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.070. What is the equilibrium constant for the reaction B(g)⇌12A(g)? 3. Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) Kp=2.91×103 at 298 K In a reaction at equilibrium, the partial pressure of SO2...

At 850.0 K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below...

At 850.0 K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below is 0.2300. N2(g)+H2(g)---> N2H2(g) If a vessel contains an initial reaction mixture in which [N2] = 0.02000 M, [H2] = 0.03000 M, and [N2H2] = 1.000×10-4 M, what will the [N2H2] be when equilibrium is reached? ________M

At 850. K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below...

At 850. K, the value of the equilibrium constant Kp for the hydrazine synthesis reaction below is 0.2100. If a vessel contains an initial reaction mixture in which [N2] = 0.02000 M, [H2] = 0.03000 M, and [N2H2] = 1.000×10-4 M, what will the [N2H2] be when equilibrium is reached?

Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...

Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) Express your answer using two significant figures. Part B O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) Express your answer using two significant figures. Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express your answer using two significant figures.

Each of the following reactions is allowed to come to equilibrium and then the volume is...

Each of the following reactions is allowed to come to equilibrium and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. Part A I2(g)⇌2I(g) (volume is increased) (volume is increased) -no effect -shifts left -shifts right Part B 2H2S(g)⇌2H2(g)+S2(g) (volume is decreased) (volume is decreased) -shifts left -no effect -shifts right Part C I2(g)+Cl2(g)⇌2ICl(g) (volume is decreased) (volume is decreased) -shifts left -shifts right -no effect

The equilibrium constant, K, for the reaction shown below has a value 1.8 x 105. In...

The equilibrium constant, K, for the reaction shown below has a value 1.8 x 105. In this reaction which is the strongest acid and which is the strongest base? CH3CO2H(aq) + H2O (l) --->H3O+(aq) + CH3CO2-(aq) please explain why?