# Chemistry

The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced.

Sb2S3(solid)+3H2(gas)<=>2Sb(solid)+3H2S(solid)

A vessel whose volume is 2.5L is filled with 0.0100 mole of antimony(III)Sulfide, Sb2S3, and 0.0100 mole H2. After the mixture came to equilibrium in a closed vessel at 440Celcius, the gaseous mixture was removed and the H2S dissolved in water. Sufficient lead(II)ion was added to react completely with H2S to precipitate lead(II)Sulfide, PbS. If 1.029g of Pbs was obtained what is the value of K(eq) at 440Celcius

k(eq)=the equilibrium constant

1. 👍
2. 👎
3. 👁
1. 1.029g PbS x (1 mol PbS/molar mass PbS)= approximately 0.004 mol but you need to calculate more carefully than that.
.......Sb2S3 + 3H2 ==> 2Sb + 3H2S
initial.0.01..0.01......0......0
change..-x......-3x.....2x....3x
equil..0.01-x..0.01-3x..2x....0.004

Therefore, H2 must be 0.01-0.004 = 0.006

I would convert 0.004 mol H2S and 0.006 mol H2 to M, substitute into the Kc expression and solve for Kc. Don't forget: solids are not part of the Kc expression. Also note the correct spelling of celsius.

1. 👍
2. 👎

## Similar Questions

1. ### Chemistry

Consider the following equilibrium process at 700°C: 2H2 + S2 ↔ 2H2S Analysis shows that there are 2.50 moles of H2, 1.35x10^-5 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate the equilibrium constant Kc

2. ### chemistry

please help and explain. At a certain temperature, Keq = 10.5 for the equilibrium below. CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g) Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing

3. ### AP Chemistry

For the system 2SO2(g) + O2(g) 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L

4. ### chemistry, plz check work

NH3+H2S-->NH4HS

1. ### Chemistry

In the industrial synthesis of ammonia, the equilibrium constant expression may be written as: Keq= [NH3]^2/[N2][H2]^3 Calculate the value of this equilibrium constant, if the equilibrium concentration of nitrogen in the reaction

2. ### Chemistry: Equilibrium

What is the significance of a very large Kp value on the equilibrium concentration of H2 in the reaction: 2H2(g) + O2(g) ->2H2O(g)?

3. ### Chemistry

SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50

4. ### Chemistry

When one mole of ammonia is heated to a given temperature, 50% of the compound dissociates and the following equilibrium is establised. NH3(g) 1/2N2(g) + 3/2H2(g) (note: is my sad attempt at the equilibrium symbol) What is the

1. ### Chemistry

What is the significance of a very large Kp value on the equilibrium concentration of H2 in the reaction : 2H2 (g) + O2 (g) 2H2O (g) ? A. There is very little H2 at equilibrium. B. There is a significant amount of H2 at

2. ### CHEMISTRY

Consider the following reaction: 2H2S+SO2=S(s)+H2O A reaction mixture initially containing 0.500M H2S and 0.500M SO2 was found to contain 1.0×10−3M at a certain temperature. A second reaction mixture at the same temperature

3. ### Chemistry

Help please, What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.350g of pure H2s(g), at 25 ∘C to achieve equilibrium? Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen

4. ### Chemistry 2

Supposed you stoppered the flasks after your titration to determine the equilibrium constant and kept the solutions for another day so that the equilibrium was re-established. What would happen to the amount of ethanol present?