Question

Solid sodium metal reacts with chlorine gas to produce solid sodium chloride in a spontaneous, exothermic reaction. a. Write and balance the equation for the reaction.

b. For the above reaction, identify: i. The oxidation state of each atom in the reactants and products: j. The species that is oxidized: k. The species that is reduced: l. The oxidizing agent: m. The reducing agent:

c. At a temperature of 30 oC and a pressure of 800 mmHg, what volume of chlorine gas would be needed to fully consume 10.5 g of sodium meta

Answer 1

C. 2Na (s) + Clz (g) → 2 Nace (s) + Cl2 (g) -> 2Nace (s) b. 2 Na (s) Oxidation. O o +1 -1 State: T oxidation oxidation : Reduction Oxidised : Na Reduced & clo Oxidising agent : Cl2 Reducing agent : Na C. Mole of Na = 10.5g = 0.4 565 mol 23glmal Mo Mole og ly = I x0.4565 = 0.22826 mol T 30°C - 303 K 1.052 6 atm 800mm Hg = fatm 760 mming PV = nRT VENRT = 0.22826 mol X 0.0821 Lamm x 303K - 1.0526 atm = 15.39 L