Question

Use the balanced equation given below to solve the problem that follows: Calculate the mass in grams of water produced along with 5.0 L of CO2 at STP.
[ ] g H2O2

2 C2H2(g) + 5 O2(g --> 4 CO2(g) + 2 H2O(g)
**Your answer should be written as X.X

Answer 1

Answer: 1.98 g

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given volume}}{\text{Molar volume}}$  

$\text{Moles of} CO_2=\frac{5.0L}{22.4L}=0.22moles$

The balanced given equation is:

$C_2H_2(g)+5O_2(g)\rightarrow 4CO_2(g)+2H_2O(g)$  

According to stoichiometry :

4 moles of $CO_2$ will produce =  2 moles of $H_2O$

Thus 0.22 moles of $CO_2$ will produce=$\frac{2}{4}\times 0.22=0.11moles$  of $H_2O$

Mass of $H_2O=moles\times {\text {Molar mass}}=0.11moles\times 18g/mol=1.98g$

Thus 1.98 g of water is produced along with 5.0 L of $CO_2$ at STP