Question

Answer the following questions based on the equation:

2Fe(s)+3Cl2(g) --> 2FeCl3(s)

a). How many moles of chlorine are needed to react with 4.0 moles of iron?

b). How many grams of iron (iii) chloride are produced by reacting 4.57 miles of chlorine with excess iron?​

Answer 1

Answer:a). According to the balanced chemical equation, 3 moles of chlorine are needed to react with 2 moles of iron.

So to calculate how many moles of chlorine are needed to react with 4.0 moles of iron, we can set up a proportion:

(3 moles of chlorine) / (2 moles of iron) = (x moles of chlorine) / (4.0 moles of iron)

Solving for x, we get:

x = (3/2) * 4.0 = 6.0 moles of chlorine

Therefore, 6.0 moles of chlorine are needed to react with 4.0 moles of iron.

b). The balanced chemical equation tells us that 2 moles of FeCl3 are produced for every 3 moles of Cl2 that react.

To calculate the number of moles of FeCl3 produced from 4.57 moles of Cl2, we can set up a proportion:

(2 moles of FeCl3) / (3 moles of Cl2) = (x moles of FeCl3) / (4.57 moles of Cl2)

Solving for x, we get:

x = (2/3) * 4.57 = 3.0467 moles of FeCl3

To convert moles of FeCl3 to grams, we need to use its molar mass. The molar mass of FeCl3 is:

FeCl3: Fe (55.85 g/mol) + 3 Cl (35.45 g/mol) = 162.2 g/mol

Therefore, the mass of FeCl3 produced is:

mass = moles * molar mass

mass = 3.0467 mol * 162.2 g/mol = 494.7 g

Therefore, 494.7 grams of iron (III) chloride are produced by reacting 4.57 miles of chlorine with excess iron.

Step-by-step explanation: