Gaseous indium dihydride is formed from the elements at elevated temperature: In(g)+H2(g)⇌InH2(g),Kp=1.48 at 973 K The...

Gaseous indium dihydride is formed from the elements at elevated temperature: In(g)+H2(g)⇌InH2(g),Kp=1.48 at 973 K The partial pressures measured in a reaction vessel are PInPH2PInH2===0.0550atm0.0290atm0.0780atm Determine the equilibrium partial pressure of In. Determine the equilibrium partial pressure of H2. Determine the equilibrium partial pressure of InH2.

Expert Solution

In(g) + H2(g) ⇌ InH2(g

I 0.055 0.029 0.078

C +x +x -x

E 0.055+x 0.029+x 0.078-x

Kp = P_InH2/P_In P_H2

1.48 = 0.078-x/(0.055+x)(0.029+x)

1.48*(0.055+x)(0.029+x) = 0.078-x

x = 0.062

P_In = 0.055+x = 0.055+0.062 =0.117atm

P_H2 = 0.029+x = 0.029+0.062 = 0.091atm

P_InH2 = 0.078-x = 0.078-0.062 = 0.016atm

queen_honey_blossom answered 2 years ago

At a certain temperature, the Kp for the decomposition of H2S is 0.714. H2S(g) <-----> H2(g)...

At a certain temperature, the Kp for the decomposition of H2S is 0.714. H2S(g) <-----> H2(g) + S(g) Initially, only H2S is present at a pressure of 0.102 atm in a closed container. What is the total pressure in the container at equilibrium?

At a certain temperature, the Kp for the decomposition of H2S is 0.785. H2S(g) to H2(g)...

At a certain temperature, the Kp for the decomposition of H2S is 0.785. H2S(g) to H2(g) + S(g) Initially, only H2S is present at a pressure of 0.142 atm in a closed container. What is the total pressure in the container at equilibrium

At a certain temperature, the Kp for the decompositon of H2S is 0.871. H2S(g) <----> H2(g)...

At a certain temperature, the Kp for the decompositon of H2S is 0.871. H2S(g) <----> H2(g) + S(g) Initally, only H2S is present at a pressure of 0.226 bar in a closed container. What is the total pressure in the container at equilibrium?

Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g)...

Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g) ⇌ 2 HI(g). Use ∆Hºrxn and ∆Sºrxn to calculate and assume that they are independent of temperature. Use the thermodynamic data in the appendix of your textbook; I have provided the needed appendix on BlackBoard for your convenience. Report your answer to zero places past the decimal.

At a certain temperature, the Kp for the decomposition of H2S is 0.842.H2S(g) H2(g) + S(g)Initially,...

At a certain temperature, the Kp for the decomposition of H2S is 0.842.H2S(g) H2(g) + S(g)Initially, only H2S is present at a pressure of 0.104 atm in a closed container. What is the total pressure in the container at equilibrium?I know: H2S(g) H2(g) + S(g) Initial: 0.104 atm 0 atm 0 atmchange: -x x xfinal: 0.104 -x x x0.842 = 0.842 = x2 + 0.842 x - 0.0876 = 0 0.109 is greater than the initial concentration of 0.104 so...

The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. H2(g) + CO2(g)...

The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. H2(g) + CO2(g) ⇌ H2O(g) + CO(g) Calculate Δ G o for the reaction. kJ/mol Calculate Δ G for the reaction when the partial pressures are PH2 = 0.22 atm, PCO2 = 0.72 atm, PH2O = 0.66 atm, and PCO = 1.16 atm.

The equilibrium constant (Kp) for the following reaction is 4.40 at 2000.K. H2(g) + CO2(g) <=>...

The equilibrium constant (Kp) for the following reaction is 4.40 at 2000.K. H2(g) + CO2(g) <=> H2O(g) + CO(g) a) Calculate Delta Go for the reaction. ____________ KJ/mol b) Calculate Delta G for the reaction when the partial pressures are PH2 = 0.28 atm, PCO2 = 0.81 atm, PH2O = 0.63 atm, and PCO = 1.17 atm. ______________ KJ/mol

23- At a certain temperature, the Kp for the decomposition of H2S is 0.820. H2S(g)<--->H2(g)+S(g) Initially,...

23- At a certain temperature, the Kp for the decomposition of H2S is 0.820. H2S(g)<--->H2(g)+S(g) Initially, only H2S is present at a pressure of 0.112 atm in a closed container. What is the total pressure in the container at equilibrium? _____atm

1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is...

1) At a certain temperature, 322 K, Kp for the reaction, Cl2(g) <=> 2 Cl(g), is 7.82 x 10-60. Calculate the value of ΔGo in kJ for the reaction at this temperature. 2) The equilibrium constant for the reaction, 2 Fe3+(aq) + Hg22+(aq) <=> 2 Fe2+(aq) + 2 Hg2+(aq) is 9.1 x 10-6(aq) at 298 K. Calculate ΔG in J when {Fe3+(aq)} = 0.375 {Hg22+(aq)} = 0.051 {Fe2+(aq)} = 0.021 {Hg2+(aq)} = 0.06

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on (a) total pressure (b) catalyst used (c) amount of H2 and I2 (d) temperature

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on___________.(a) total pressure(b) catalyst used(c) amount of H2 and I2(d) temperature

Question