Preview - Ideal Gas Laws - Connected Chemistry 2019

The ideal gas law: making the theory work


Let's review how we would put together our three theories mathematically:

Step 1: We would write them one by one:

\(P = m_1 \times N\)     (Eq. 1)

\(P = m_2 \times T\)     (Eq. 2)

\(P = {m_3 \over V}\)     (Eq. 3)

 

Step 2: We would combine the right side of the equations:

\(P = {{(m_1 \times N) \times (m_2 \times T) \times (m_3)} \over V}\)     (Eq. 4)

 

Step 3: We would slightly modify the equation by moving \(V\) to the other side of the equation and we would also get rid of the parentheses:

\(P \times V = {m_1 \times m_2 \times m_3 \times N \times T }\)     (Eq. 5)

 

Finally, we would combine all three coefficients \((m_1 \times m_2 \times m_3)\)as one coefficient, which we can simply call as \(m_g\) or the ideal gas coefficient:

\(P \times V = {m_g \times N \times T }\)     (Eq. 6)


Questions

Please answer the questions below.

In the field of chemistry, our model is expressed slightly differently as \(P \times V = n \times R \times T\), where

  • \(n\) corresponds to \(N\) or "number of particles" in our model, expressed in moles
  • \(R\)  corresponds to \(m\)  or "gas coefficient" in our model, which is called the "universal gas constant." 
    • Its value is 0.08 L atm / mol K.

 

Answer the following chemistry problem using the ideal gas equation:

5 moles of nitrogen gas is in a 100 liter fixed cylinder at 300 Kelvin. 
What is the pressure of the gas?

Note: please determine the values of each of your independent variables (e.g., volume, temperature) and fill the data table below.


Also answer the textbook question below:

Note: The temperature of air inside our lungs is approximately 37o C (273 + 37 = 310o K)


Please describe how you solved the question above. Explain in steps. (min. 3 steps). 

Such as:

  • First, we did ....
  • Then we did ....
  • ....

Optional question if you finished early: Answer the (b) part of the textbook question below. Also explain how you solved this problem.


Notes

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