D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO₂ will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl (aq) → H₂O (1) +CaCl₂ (aq) + CO₂ (g)
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.
![## Chemistry Problem Set
### Problem 19:
Given: 68.1 g of solid CaCO₃ is mixed with excess HCl. Determine the volume of CO₂ collected at 0.0°C and 1 atm. (Molar mass: CaCO₃ = 100.08 g/mol, CO₂ = 44.1 g/mol)
Equation:
\[ \text{CaCO}_3 (s) + 2 \text{HCl} (aq) \rightarrow \text{H}_2\text{O} (l) + \text{CaCl}_2 (aq) + \text{CO}_2 (g) \]
**Options:**
- (A) **15.2 L**
- (B) 0
- (C) +3
- (D) +7
**Correct Answer: (A) 15.2 L**
### Problem 20:
A gas sample has an initial volume of 0.500 L and an initial pressure of 1.0 atm. What is the volume when the pressure of the sample is decreased to 0.50 atm? Assume the temperature and number of moles of the gas are constant.
**Options:**
- (A) 0 L
- (B) **0.99 L**
- (C) 0.025 L
- (D) 155 L
**Correct Answer: (B) 0.99 L**
### Explanation:
For the first problem, the given chemical reaction is used to calculate the number of moles of CO₂ produced and then the volume using the ideal gas law.
In the second problem, Boyle's Law (P₁V₁ = P₂V₂) is used to find the new volume of the gas when the pressure changes while keeping the temperature constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffddc283e-bfa7-4492-b564-1add28da6d82%2F9035b339-eaae-4bfe-ad0f-06b029fe4e7d%2Fm6l4vu_processed.jpeg&w=3840&q=75)
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