Question

In the reaction: 2Na(s) + Cl2(g) → 2NaCl(g) If 53.2 g Na reacts with 65.8 g Cl₂, What the theoritical yield of NaCl is formed

A 80.9
B 106 g
C 25.7
D 66.5
E none of these

Answer 1

First, calculate the molar mass of each substance:

Na: 22.99 g/mol
Cl2: 35.45 g/mol
NaCl: 22.99 + 35.45 = 58.44 g/mol

Next, determine the number of moles of each substance:

Moles of Na: 53.2 g / 22.99 g/mol = 2.31 mol
Moles of Cl2: 65.8 g / 35.45 g/mol = 1.86 mol

From the balanced equation, we can see that 2 moles of NaCl are produced for every 2 moles of Na:

Moles of NaCl produced from Na: 2.31 mol x (2 mol NaCl / 2 mol Na) = 2.31 mol

Since the moles of Cl2 are limiting, only 1.86 moles of NaCl can be produced.
Convert this to grams:

Theoretical yield of NaCl = 1.86 mol x 58.44 g/mol = 108.5 g

The closest answer choice is 106 g, so the correct answer is B) 106 g.