Question #f51ce

1 Answer
Sep 11, 2017

Answer:

At STP, the volume of chlorine used is 90.9 L.

Explanation:

There are four steps involved in this stoichiometry problem:

Step 1. Write the balanced chemical equation.

#M_r:color(white)(mmmmmmm) 36.46#
#color(white)(mmm)"H"_2 + "Cl"_2 → "2HCl"#

2. Convert grams of #"HCl"# to moles of #"HCl"#

#"Moles of HCl" = 292 color(red)(cancel(color(black)("g HCl"))) × ("1 mol HCl")/(36.46 color(red)(cancel(color(black)("g HCl")))) = "8.009 mol HCl"#

Step 3. Convert moles of #"HCl"# to moles of #"Cl"_2#

#"Moles of Cl"_2 = 8.009color(red)(cancel(color(black)("mol HCl"))) × ("1 mol Cl"_2)/(2 color(red)(cancel(color(black)("mol HCl")))) = "4.004 mol Cl"_2#

4. Calculate the volume of #"Cl"_2#

At STP (1 bar and 0 °C), the molar volume of a gas is 22.71 L.

#V = 4.004 color(red)(cancel(color(black)("mol"))) × "22.71 L"/(1 color(red)(cancel(color(black)("mol")))) = "90.9 L"#

The volume of #"Cl"_2# used is 90.9 L.

Here's a useful video on mass-volume conversions.