2. Decomposition of H2O2 is shown below 2 H202 (1) → 2 H20(1) + 02(g) At the end of the reaction, 0.75 L of gas was collected over water at 25 °C and the total pressure measured was 766 mm Hg. How many moles of H2O2 were consumed by the reaction? Given: vapor pressure of water at 25 °C = 24 mm Hg 1 atm = 760. mm Hg R = 0.0821 atm L mole' K! H:O2 =34.0158 g/mole
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![**Educational Content: Chemistry Problem Solving**
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**Decomposition of Hydrogen Peroxide**
The decomposition reaction of hydrogen peroxide (\(H_2O_2\)) is represented as follows:
\[
2 \text{H}_2\text{O}_2(l) \rightarrow 2 \text{H}_2\text{O}(l) + \text{O}_2(g)
\]
At the end of this reaction, 0.75 L of oxygen gas was collected over water at 25°C. The total pressure measured was 766 mm Hg. Calculate the moles of \(H_2O_2\) consumed in the reaction.
**Given:**
- **Vapor pressure of water at 25°C**: 24 mm Hg
- **Conversions and constants**:
- \(1 \text{ atm} = 760 \text{ mm Hg}\)
- \(R = 0.0821 \text{ atm} \cdot \text{L} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}\)
- Molar mass of \(H_2O_2\): 34.0158 g/mol
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**Sodium Hydroxide Dissolution**
Sodium hydroxide (NaOH) with a mass of 4.00 g and water with a mass of 100.0 g are initially at 20.0°C. Upon dissolving the NaOH in a coffee cup calorimeter, the solution's temperature increases to 29.6°C. The specific heat of the solution is 3.98 J/g°C. Using NaOH as the limiting reactant, determine the molar enthalpy of solvation in kJ/mol.
**Note:**
This problem involves using concepts like stoichiometry, gas laws, and calorimetry. Ensure unit conversions are consistent, and apply the appropriate equations to solve for the unknowns.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8952ab44-c2b4-44e3-abe0-9c4c6278d60a%2F67d0e1bf-3efc-4489-838f-9825aeb1c35e%2F9guotbc_processed.jpeg&w=3840&q=75)
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