What do they mean by accepted molar mass of butane in question #7? I've calculated the molar mass of butane gas and found that it was 0.574 g/mol because I found the mass of the butane (0.1027 g) and divided it by the number of moles of butane (0.179 mol).
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
What do they mean by accepted molar mass of butane in question #7? I've calculated the molar mass of butane gas and found that it was 0.574 g/mol because I found the mass of the butane (0.1027 g) and divided it by the number of moles of butane (0.179 mol).
![**Educational Resource: Experimental Determination of Molar Mass of Butane**
**Data Table:**
A table is presented with the following columns:
1. **Trial Number**: (1, 2, 3)
2. **Lighter Number**: (Blank rows)
3. **Initial Mass of Lighter** (g):
- 13.5099
- Blank
- Blank
4. **Final Mass of Lighter** (g):
- 12.0482
- Blank
- Blank
- (Note: "we’ll get this after they have dried overnight")
5. **Temperature** (°C) (Reads from the thermometer):
- 22.4
- Blank
- Blank
6. **Volume of Butane** (mL) (Reads from eudiometer tube):
- 448
- 2
- Blank
7. **Barometric Pressure** (inHg) (Reads from barometer):
- 29.85
- Blank
- Blank
8. **Vapor Pressure of Water** (Reads from chart of vapor pressures):
- 20.45
- Blank
- Blank
**Analysis:**
1. **Convert** the barometric pressure from inHg to mmHg. (1 in = 25.4 mm).
2. **Use Dalton’s Law** to calculate the pressure of the butane alone.
3. Using the **Ideal Gas Law**, calculate the moles of butane for each trial using the formula:
\[ PV = nRT \]
4. **Calculate** the mass of butane collected for each trial.
5. **Calculate** the molar mass of butane for each trial using:
\[ \text{Molar Mass} = \frac{\text{Mass}}{\# \text{ of moles}} \]
6. **Calculate** the average molar mass of butane.
7. **Determine** the formula of butane and calculate the percent error in your experimentally determined molar mass.
8. If some bubbles of butane escape and are not collected in the eudiometer, how will the experimentally determined molar mass be affected?
9. If an air bubble is left in the eudiometer before the gas is collected, how will the experimentally determined molar mass be](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a487c5b-631b-4d04-995d-e7c019732a55%2F9a56e28b-ddc0-47f3-a6d3-2e90f8f1460c%2F3hsmte_processed.jpeg&w=3840&q=75)
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So would 0.547 g/mol not be the experimental molar mass?
by Bartleby ExpertWhere did the number 0.001316 atm come from?
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