Question

Consider the following reaction: 2 H2S (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2H2 (g) + S 2 (g) Which answer represents the equilibrium constant for this reaction?

The concentration of H subscript two to the exponent 2 multiplied by the concentration of S2 in the numerator all over the concentration of H2S to the exponent 2 in the denominator.
The concentration of H subscript two multiplied by the concentration of S2 in the numerator all over the concentration of H subscript two S in the denominator.
Two times the concentration of H subscript two multiplied by the concentration of S subscript two in the numerator all over two times the concentration of H subscript two S in the denominator.
The concentration of Hsubscript two S to the exponent 2 in the numerator all over the concentration of H subscript two multiplied by the concentration of S subscript two in the denominator.

Answer 1

Answer: The concentration of H subscript two to the exponent 2 multiplied by the concentration of S2 in the numerator all over the concentration of H2S to the exponent 2 in the denominator.

Step-by-step explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

`2H_2S(g)\rightarrow 2H_2(g)+S_2(g)`

The equilibrium constant in terms of concentration is written as :

`K_c=([H_2]^2* [S_2])/([H_2S]^2)`

The numerals written below the symbols are subscripts and the numerals above are called as exponents.

Thus the concentration of H subscript two to the exponent 2 multiplied by the concentration of
`S_2` in the numerator all over the concentration of
`H_2S` to the exponent 2 in the denominator.

Answer 2

The concentration of H subscript two to the exponent 2 multiplied by the concentration of S2 in the numerator all over the concentration of H2S to the exponent 2 in the denominator

Step-by-step explanation:

Equilibrium is a state wherein the rate at which the reactants disappear equals the rate at which the products are formed. In other words, at equilibrium the concentrations of the reactants and products remain unchanged. This state is defined by a constant known as the equilibrium constant (Keq) which is the ratio of the concentration of the products over the reactants.

The given reaction is the decomposition of H2S into H2 and S:

`2H_(2)S(g)\rightleftharpoons 2H_(2)(g)+ S_(2)(g)`

The equilibrium constant is given as:

`Keq = ([H_(2)]^(2)[S_(2)])/([H_(2)S]^(2))`