Question
A.Define temperature and state it's SI unit.
B. Current 100 kelvin into degree Celsius and Fahrenheit
C. Convert 5 degree Celsius into kelvin
D. How hot wile a 2.3 litres balloon have to get to expand to a volume of 400 litres? Assume that the initial temperature of the balloon is 25 degree Celsius
B. Current 100 kelvin into degree Celsius and Fahrenheit
C. Convert 5 degree Celsius into kelvin
D. How hot wile a 2.3 litres balloon have to get to expand to a volume of 400 litres? Assume that the initial temperature of the balloon is 25 degree Celsius
Answers
GPT-4o mini
### A. Definition of Temperature
**Temperature** is a physical quantity that indicates the degree of hotness or coldness of a system. It is a measure of the average kinetic energy of the particles in a substance. Temperature is a fundamental parameter in various scientific and engineering fields and plays a crucial role in thermodynamics.
**SI Unit**: The SI unit of temperature is the **Kelvin (K)**.
---
### B. Current 100 Kelvin into Degree Celsius and Fahrenheit
To convert Kelvin to degrees Celsius:
\[
°C = K - 273.15
\]
\[
°C = 100 - 273.15 \approx -173.15°C
\]
To convert from degrees Celsius to Fahrenheit:
\[
°F = (°C \times \frac{9}{5}) + 32
\]
\[
°F = (-173.15 \times \frac{9}{5}) + 32 \approx -279.67°F
\]
**Result**:
- 100 K ≈ -173.15 °C
- 100 K ≈ -279.67 °F
---
### C. Convert 5 Degrees Celsius into Kelvin
To convert Celsius to Kelvin:
\[
K = °C + 273.15
\]
\[
K = 5 + 273.15 = 278.15 \, K
\]
**Result**: 5 °C = 278.15 K
---
### D. How Hot Will a 2.3 Litres Balloon Have to Get to Expand to a Volume of 400 Litres?
Assuming the balloon behaves ideally, we can use the ideal gas law or Charles' law for this calculation. Charles' law states that the volume of a gas is directly proportional to its temperature (in Kelvin) when pressure is constant.
The formula can be given as:
\[
\frac{V_1}{T_1} = \frac{V_2}{T_2}
\]
Where:
- \( V_1 \) = initial volume = 2.3 L
- \( V_2 \) = final volume = 400 L
- \( T_1 \) = initial temperature in Kelvin = \( 25 \,°C + 273.15 = 298.15 \, K \)
- \( T_2 \) = final temperature in Kelvin (unknown)
Rearranging the equation to solve for \( T_2 \):
\[
T_2 = T_1 \cdot \frac{V_2}{V_1}
\]
Now substituting in the values:
\[
T_2 = 298.15 \cdot \frac{400}{2.3}
\]
Calculating:
\[
T_2 = 298.15 \cdot 173.913 \approx 51749.2 \, K
\]
This result is extremely high and indicates that the balloon would need an impractically high temperature to achieve such an expansion under the assumptions listed.
**Result**: The temperature required for the balloon to expand from 2.3 litres to 400 litres, starting from an initial temperature of 25 °C, is approximately \( 51749.2 \, K \).
**Temperature** is a physical quantity that indicates the degree of hotness or coldness of a system. It is a measure of the average kinetic energy of the particles in a substance. Temperature is a fundamental parameter in various scientific and engineering fields and plays a crucial role in thermodynamics.
**SI Unit**: The SI unit of temperature is the **Kelvin (K)**.
---
### B. Current 100 Kelvin into Degree Celsius and Fahrenheit
To convert Kelvin to degrees Celsius:
\[
°C = K - 273.15
\]
\[
°C = 100 - 273.15 \approx -173.15°C
\]
To convert from degrees Celsius to Fahrenheit:
\[
°F = (°C \times \frac{9}{5}) + 32
\]
\[
°F = (-173.15 \times \frac{9}{5}) + 32 \approx -279.67°F
\]
**Result**:
- 100 K ≈ -173.15 °C
- 100 K ≈ -279.67 °F
---
### C. Convert 5 Degrees Celsius into Kelvin
To convert Celsius to Kelvin:
\[
K = °C + 273.15
\]
\[
K = 5 + 273.15 = 278.15 \, K
\]
**Result**: 5 °C = 278.15 K
---
### D. How Hot Will a 2.3 Litres Balloon Have to Get to Expand to a Volume of 400 Litres?
Assuming the balloon behaves ideally, we can use the ideal gas law or Charles' law for this calculation. Charles' law states that the volume of a gas is directly proportional to its temperature (in Kelvin) when pressure is constant.
The formula can be given as:
\[
\frac{V_1}{T_1} = \frac{V_2}{T_2}
\]
Where:
- \( V_1 \) = initial volume = 2.3 L
- \( V_2 \) = final volume = 400 L
- \( T_1 \) = initial temperature in Kelvin = \( 25 \,°C + 273.15 = 298.15 \, K \)
- \( T_2 \) = final temperature in Kelvin (unknown)
Rearranging the equation to solve for \( T_2 \):
\[
T_2 = T_1 \cdot \frac{V_2}{V_1}
\]
Now substituting in the values:
\[
T_2 = 298.15 \cdot \frac{400}{2.3}
\]
Calculating:
\[
T_2 = 298.15 \cdot 173.913 \approx 51749.2 \, K
\]
This result is extremely high and indicates that the balloon would need an impractically high temperature to achieve such an expansion under the assumptions listed.
**Result**: The temperature required for the balloon to expand from 2.3 litres to 400 litres, starting from an initial temperature of 25 °C, is approximately \( 51749.2 \, K \).