Lead metal is added to 0.140M Cr^+3(aq).
Pb(s)+ 2Cr^3+(aq)---> Pb^2+(aq) + 2Cr^2+(aq)
a)What is [Pb^2+] when equilibrium is established in the reaction?
b)What is [Cr^2+] when equilibrium is established in the reaction?
c)What is [Cr^3+] when equilibrium is established in the reaction?
To solve this problem, we need to use the concept of balancing chemical equations and the principles of equilibrium. Here's how we can find the answers:
a) To determine [Pb^2+] at equilibrium, we need to consider the stoichiometry of the balanced chemical equation. According to the equation, one mole of lead (Pb) reacts with two moles of Cr^3+. So, if x moles of Pb^2+ are formed, then 2x moles of Cr^3+ must react.
Since the initial concentration of Cr^3+ is 0.140 M, the change in concentration of Cr^3+ is 2x M. Therefore, the equilibrium concentration of Cr^3+ is 0.140 - 2x M.
Using the law of conservation of mass, we can conclude that the equilibrium concentration of [Pb^2+] is also x M.
b) Similarly, if x moles of Pb^2+ are formed, then 2x moles of Cr^3+ must react. Hence, the equilibrium concentration of Cr^2+ is also 2x M.
c) The initial concentration of Cr^3+ is 0.140 M. Since we assume that all of the Cr^3+ reacts, the change in concentration would be 2x M. Consequently, the equilibrium concentration of Cr^3+ is 0.140 - 2x M.
To find the values of x, we need more information, such as the initial amount of lead (Pb) added or some other data related to the reaction conditions. Once we have this information, we can set up an expression for the equilibrium constant (K) and solve for x using the equation for K.
Let me know if you have any further information or if you would like to proceed with solving for the values of x.