Astudent is asked to balance an equation by using the half-reaction method. he determines the two half reactions as shown below. 2br- ➡️ br2+2e- cl2+2e-➡️2cl- what should he write as the final, balances equation ? cl2 +2br-➡️br2+2cl- cl2+2br-+2e-➡️br2+2cl- cl2+2br-➡️br2 +cl- + 2e- cl2 +br-+2e-➡️br2+cl-+2e-

2Br ⁻ ➡️ Br2+2e-

Cl2+2e-➡️2Cl⁻

Cl2 +2Br⁻➡️Br2 +2Cl⁻

Answer A.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

first one is the correct answer