Suppose you performed a similar experiment using an unknown carbonate sample. The pressure and volume were measured after the temperature stabilized at 21.5 °C. Given the data in the table, calculate the moles of CO₂ produced. initial pressure (atm) initial gas volume (mL) volume of 1.0 M HCI solution added to fully consume the carbonate sample (ml) moles of CO₂: 18.33 PV=nRT Incorrect final pressure (atm) final gas volume (mL) What is the stoichiometric ratio between HCI and CO₂? n=PV/RT=1.32*0.022/0.0821*294.5-0.0012moles stoichiometric ratio between HCI and CO2=0.022/0.0012-18.33 1.000 240.0 22.0 2.320 218.0 mol
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.
![Suppose you performed a similar experiment using an unknown carbonate sample. The pressure and volume were measured after the temperature stabilized at 21.5°C. Given the data in the table, calculate the moles of CO₂ produced.
| Measurement | Value |
|--------------------------------------------------|----------------|
| Initial pressure (atm) | 1.000 |
| Initial gas volume (mL) | 240.0 |
| Volume of 1.0 M HCl solution added (mL) | 22.0 |
| Final pressure (atm) | 2.320 |
| Final gas volume (mL) | 218.0 |
**Moles of CO₂:**
The initial attempt to calculate the moles of CO₂ resulted in "18.33 mol," which is incorrect.
**Calculating the Stoichiometric Ratio:**
What is the stoichiometric ratio between HCl and CO₂?
Using the ideal gas law:
\[ PV = nRT \]
Given:
- \( P = 1.32 \, \text{atm} \)
- \( V = 0.022 \, \text{L (converted from 22.0 mL)} \)
- \( R = 0.0821 \, \left(\text{L atm/mol K}\right) \)
- \( T = 294.5 \, \text{K} \, (21.5 + 273) \)
The calculation:
\[ n = \frac{PV}{RT} = \frac{1.32 \times 0.022}{0.0821 \times 294.5} = 0.0012 \, \text{moles} \]
The stoichiometric ratio between HCl and CO₂ is:
\[ = \frac{0.022}{0.0012} = 18.33 \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ddfe527-492b-49f8-bf31-fc2086d1cdeb%2F293dccee-3619-43c2-81f2-d901907cc63c%2F4n58kzi7_processed.jpeg&w=3840&q=75)
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