What is the mass of water vapour produced?

enter image source here

1 Answer
Dwight
Jan 4, 2018

This problem combines the ideal gas law and stoichiometry t show that 3.78 g of #H_2O# are produced. The solution follows...

Explanation:

First, we must determine the number of moles of #CO_2# produced, because a chemical equation demands all quantities be in moles.

The ideal gas law will help us here:

#PV=nRT#

where #R# is the gas constant, 8.314 kPa L/ mol K. We solve for #n#:

#n = (PV)/(RT) = ((100 kPa)(5L))/((8.314)(573 K))=0.105# mol of #CO_2#

(Note the conversion of Celsius temperature to Kelvin)

Now, we can apply the chemical equation, which tells us that the quantity of #H_2O# produced is twice the amount of #CO2#, which we get from the coefficients to the left of these substances.

#"mol " H_2O= "mol "CO_2 xx 2 = 0.210# mol #H_2O#

Since the molar mass of #H_2O# is 18 g, the mass of #H_2O# produced is

#0.210 "mol" xx 18.0 g/(mol) = 3.78 g#

Related questions
Impact of this question
3890 views around the world
You can reuse this answer
Creative Commons License