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

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} CO_2=(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=
`(2)/(4)* 0.22=0.11moles` of
`H_2O`

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

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