A cylinder contains 10 grams of Nitrogen gas initially at a pressure of 20,000 Pa.  Heat flows into the system, which causes the temperature to rise from 40oC to 60oC. 

First, write the equation for the ideal gas law

The **ideal gas law** is expressed as:

\[
PV = nRT
\]

where:
- \(P\) is the pressure of the gas (in Pascals, Pa),
- \(V\) is the volume of the gas (in cubic meters, m³),
- \(n\) is the number of moles of the gas (in moles),
- \(R\) is the ideal gas constant (\(R = 8.314 \, \text{J/mol·K}\)),
- \(T\) is the temperature of the gas (in Kelvin, K).

### Note:
To use this law, the temperature should be in Kelvin, and the amount of gas should be expressed in moles.

Would you like to proceed with solving this problem using the ideal gas law, or do you have another step in mind? 

### Related Questions:
1. How do you convert Celsius to Kelvin?
2. What is the value of the gas constant \(R\) in different units?
3. How do you calculate the number of moles from a given mass of gas?
4. What changes occur in a gas when it is heated at constant volume?
5. How does the ideal gas law apply to real gases at high pressures?

### Tip:
Always convert temperatures to Kelvin before using the ideal gas law by adding 273.15 to the Celsius temperature.

A cylinder contains 10 grams of Nitrogen gas initially at a pressure of 20,000 Pa. Heat flows into the system, which causes the temperature to rise from 40°C to 60°C. First, write the equation for the ideal gas law.

Explore the application of the ideal gas law to solve a problem involving 10 grams of Nitrogen gas at an initial pressure of 20,000 Pa. Learn how to convert temperature from Celsius to Kelvin and calculate the number of moles from the given mass. Suitable for students in Grades 9-12.

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