Respuesta :
1) Write the chemical equation.
[tex]CH_4+2O_2\rightarrow CO_2+2H_2O[/tex]2) List the known and unknown quantities.
Sample: 2.7 g CH4.
Temperature: 380 K.
Pressure: 1.5 atm.
3) Convert grams of CH4 to moles of CH4.
The molar mass of CH4 is 16.0425 g/mol.
[tex]mol\text{ }CH_4=2.7\text{ }g\text{ }CH_4*\frac{1\text{ }mol\text{ }CH_4}{16.0425\text{ }g\text{ }CH_4}=0.17\text{ }mol\text{ }CH_4[/tex]4) Moles of H2O produced from 0.17 mol CH4.
The molar ratio between CH4 and H2O is 1 mol CH4: 2 mol H2O.
[tex]mol\text{ }H_2O=0.17\text{ }CH_4*\frac{2\text{ }mol\text{ }H_2O}{1\text{ }mol\text{ }CH_4}=0.34\text{ }H_2O[/tex]5) Volume of H2O produced in the reaction.
5.1- List the known and unknown quantities.
Moles: 0.34 mol H2O.
Temperature: 380 K.
Pressure: 1.5 atm.
Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1)
5.2- Set the equation.
[tex]PV=nRT[/tex]5.3- Plug in the known values and solve for V (liters).
[tex](1.5\text{ }atm)*(V)=(0.34\text{ }mol\text{ }H_2O)*(0.082057\text{ }L*atm*K^{-1}*mol^{-1})*(380\text{ }K)[/tex][tex]V=\frac{(0.34\text{ }mol\text{ }H_2O)(0.082057\text{ }L*atm*K^{-1}*mol^{-1})(380\text{ }K)}{1.5\text{ }atm}[/tex][tex]V=7.1\text{ }L[/tex]7.1 L H2O was produced from 2.7 g CH4 in the reaction.
