Methane and Hydrogen Sulfide react at 960 degree Celsius and come to the following equilibrium
CH4(g)+2H2S(g) <-> CS2(g)+ 4H2(g)
At Equilibrium the concentration measured as
[Ch4]= 5.56M
[H2s]= 11.12
[CS2]= 2.44M
[H2] 1.76,
A) Write the equilibrium constant expression
Calquate Keq at 960 degree celcius
C)What is the effect of adding more H2 to the equilbrium mixture
D) what is the effect of increasing the volume of the container
You need to learn how to do these. What is your main problem; i.e., what is it you don't understand about these four questions? I believe you know all but one or two small items.
A And B are my main problems
Keq = (right side)/(left side) with coefficients becoming exponents.
Plug in the concns listed and punch the calculator.
A) The equilibrium constant expression, Kc, is written by using molar concentrations of the reactants and products, each raised to the power of their respective stoichiometric coefficients in the balanced equation.
For the reaction:
CH4(g) + 2H2S(g) ⇌ CS2(g) + 4H2(g)
The equilibrium constant expression would be:
Kc = ([CS2] * [H2]^4) / ([CH4] * [H2S]^2)
B) To calculate the equilibrium constant (Keq) at 960 degrees Celsius, you need to use the concentrations provided in the question. Simply substitute those values into the equilibrium constant expression and calculate Keq.
Given:
[CH4] = 5.56 M
[H2S] = 11.12 M
[CS2] = 2.44 M
[H2] = 1.76 M
Substituting these values into the equilibrium constant expression:
Keq = (2.44 * (1.76)^4) / (5.56 * (11.12)^2)
Calculate the expression using a calculator to get the numerical value of Keq.
C) Adding more H2 to the equilibrium mixture would shift the equilibrium position towards the products (CS2 and H2). According to Le Chatelier's principle, an increase in the concentration of one of the reactants will favor the formation of the products to restore equilibrium.
D) Increasing the volume of the container has an effect on the equilibrium only if the number of moles of gas changes due to the reaction. In this case, the overall number of moles of gas remains the same. Therefore, increasing the volume of the container will not have a significant effect on the equilibrium position or the concentrations of the reactants and products.