Question

СРОЧНО! Складіть математичні вирази для швидкостей прямої і зворотньої реакцій, а також для константи рівноваги наступної системи. В якому напрямі зміститься рівновага цієї системи при зміні умов? CO2(г) + Н2(г) CO(г) + H2O(г) А) при зниженні концентрації CO; б) при зниженні тиску.

Answer 1

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Answer 2

Mathematical Expressions for Reaction Rates and Equilibrium Constant

To express the reaction rates and equilibrium constant for the given system, we can use the rate law and the equilibrium expression.

The rate law for a reaction is an equation that relates the rate of the reaction to the concentrations of the reactants. It is usually determined experimentally. The general form of a rate law for a reaction is:

Rate = k[A]^m[B]^n

Where: - Rate is the rate of the reaction - k is the rate constant - [A] and [B] are the concentrations of the reactants A and B, respectively - m and n are the reaction orders with respect to reactants A and B, respectively

The equilibrium constant (K) for a reaction is a measure of the extent to which the reactants are converted into products at equilibrium. For the given reaction, the equilibrium constant expression can be written as:

K = [CO]^a[H2O]^b / [CO2]^c[H2]^d

Where: - [CO], [H2O], [CO2], and [H2] are the concentrations of CO, H2O, CO2, and H2, respectively - a, b, c, and d are the stoichiometric coefficients of CO, H2O, CO2, and H2, respectively, in the balanced chemical equation

Direction of Equilibrium Shift

The direction in which the equilibrium of a reaction shifts when conditions are changed depends on Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust to counteract the change and restore equilibrium.

In the given system, the reaction is:

CO2(g) + H2(g) ⇌ CO(g) + H2O(g)

A) When the concentration of CO decreases:

According to Le Chatelier's principle, if the concentration of a reactant is decreased, the equilibrium will shift in the direction that produces more of that reactant. In this case, if the concentration of CO decreases, the equilibrium will shift to the right to produce more CO to restore the balance.

B) When the pressure decreases:

In a gaseous reaction, if the pressure is decreased, the equilibrium will shift in the direction that produces more moles of gas. In this case, the reaction produces a total of 3 moles of gas on the left side (CO2 and H2) and 2 moles of gas on the right side (CO and H2O). Therefore, if the pressure decreases, the equilibrium will shift to the left to produce more moles of gas and restore the balance.

Note: The direction of equilibrium shift in response to changes in temperature cannot be determined without additional information.

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