We have the decomposition reaction of water that is described by the following balanced equation:
[tex]2H_2O\rightarrow2H_2+O_2[/tex]
To solve the question we will follow the following steps.
1. We find the moles of O2 formed from the ideal gas law that tells us:
[tex]PV=nRT[/tex]
Where,
P is the pressure of the gas, 0.993atm
V is the volume of the gas, 1.4L
T is the temperature of the gas, 323K
R is a constant, 0.08206atm-L/mol.K
n is the number of moles
We clear the number of moles and replace the known data:
[tex]\begin{gathered} n=\frac{PV}{RT} \\ n=\frac{0.993atm\times1.4L}{0.08206\frac{atm.L}{mol.K}\times323K}=0.052molO_2 \end{gathered}[/tex]
2. We find the moles of H2O needed from the stoichiometry of the reaction. Two moles of water produce one mol of O2, so the ratio H2O to O2 is 2/1.
[tex]\begin{gathered} MolH_2O=0.052molO_2\times\frac{2molH_2O}{1molO_2} \\ MolH_2O=0.10molH_2O \end{gathered}[/tex]
Answer: Are required 0.10mol of H2O
