Respuesta :
Answer:
The pressure in the container is 4.685atm.
Explanation:
1st) It is necessary to write and balance the chemical reaction:
[tex]C_2H_4+3O_2\rightarrow2CO_2+2H_2O[/tex]Now we know that 1 mole of C2H4 reacts with 3 moles of O2 to produce 2 moles of CO2 and 2 moles of H2O.
Using the molar mass of C2H4 (28.05g/mol) and the molar mass of CO2 (44.01g/mol) we can convert moles to grams.
So, according to the balanced reaction 28.05g of C2H4 produce 88.02g of CO2 (2 moles x 44.01 g/mol).
2nd) Now we can calculate the grams of CO2 that will be produced from 27.4g of C2H4, using a mathematical rule of three:
[tex]\begin{gathered} 28.05gC_2H_4-88.02gCO_2 \\ 27.4gC_2H_4-x=\frac{27.4gC_2H_4*88.02gCO_2}{28.05gC_2H_4} \\ x=85.98gCO_2 \end{gathered}[/tex]Now we know that 85.98g of CO2 are collected.
3rd) With the molar mass of CO2 (44.01g/mol) we can convert 85.98g into moles:
[tex]85.98g*\frac{1mol}{44.01g}=1.95moles[/tex]Now we know that there are 1.95 moles of CO2 (n).
4th) Finally, to calculate the pressure we have to replace the values of volume (V), temperature (T), moles (n) and the constant gas (R=0.082 atm*L/mol*K) in the Ideal Gases formula.
Remember that to use the Ideal Gases formula the units must be atm, liters, mol and Kelvin.
The given information from the exercise is:
- Volume (V): 10.0L
- Temperature (T): 20°C (293K)
Replacing in the formula:
[tex]\begin{gathered} P*V=n*R*T \\ P*10.0L=1.95mol*0.082\frac{atm*L}{mol*K}*293K \\ P*10.0L=46.85atmL \\ P=\frac{46.85atmL}{10.0L} \\ P=4.685atm \end{gathered}[/tex]So, the pressure in the container is 4.685atm.
