Water undergoes hydrolysis according to the following formula: 2H₂O + $\rightarrow$ O₂ + 2H₂
If the hydrogen produced is captured in a glass tube, and the hydrogen captured measures 5.00 mL then how many molecules of water would have undergone electrolysis, when the pressure inside the tube is 1 atm at a temperature of 22.0˚C? The vapor pressure of water at 22.0˚C is 19.84 mmHg.

Question

Water undergoes hydrolysis according to the following formula: 2H₂O +

\rightarrow

O₂ + 2H₂
If the hydrogen produced is captured in a glass tube, and the hydrogen captured measures 5.00 mL then how many molecules of water would have undergone electrolysis, when the pressure inside the tube is 1 atm at a temperature of 22.0˚C? The vapor pressure of water at 22.0˚C is 19.84 mmHg.

Quizplus · Accepted Answer

To find the number of molecules of water that underwent electrolysis, we first need to calculate the amount of hydrogen gas produced in moles. We can use the ideal gas law for this purpose: $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles, $R$ is the ideal gas constant, and $T$ is the temperature in Kelvin.Given:- Volume ($V$) = 5.00 mL = 0.005 L (since 1 mL = 0.001 L)- Pressure ($P$) = 1 atm - (19.84 mmHg in atm) = 1 atm - (19.84/760 atm) ≈ 0.9739 atm (since 1 atm = 760 mmHg)- Temperature ($T$) = 22.0˚C = 295.15 K (since $T(K) = T(˚C) + 273.15$)- Ideal gas constant ($R$) = 0.0821 L·atm/(mol·K)Rearranging the ideal gas law to solve for $n$, we get $n = \frac{PV}{RT}$.Substituting the given values:$$n = \frac{(0.9739 \, \text{atm}) \times (0.005 \, \text{L})}{(0.0821 \, \text{L·atm/(mol·K)}) \times (295.15 \, \text{K})}$$$$n ≈ 0.000210 \, \text{mol}$$Since the question asks for the number of water molecules that underwent electrolysis, and the reaction shows that 2 molecules of water produce 2 molecules of hydrogen, the moles of water undergoing electrolysis would be approximately the same as the moles of hydrogen produced, which is 0.000210 mol. Therefore, the correct answer is A) 0.000210 mol.

Water Undergoes Hydrolysis According to the Following Formula: 2H2O →\rightarrow→ O2 + 2H2 If the Hydrogen Produced Is Captured in \rightarrow

Water Undergoes Hydrolysis According to the Following Formula: 2H₂O $\rightarrow$ O₂ + 2H₂
If the Hydrogen Produced Is Captured in \rightarrow