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The graph you provided shows a plot of pressure (in psi) versus volume (vol), with a curve fit that follows the equation \( y = Ax^B \), where the coefficients are \( A = 843.93 \) and \( B = -0.92683 \). This type of relationship, where pressure decreases as volume increases in a power-law form, is characteristic of **Boyle's Law**.

**Boyle's Law** states that for a fixed amount of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume. Mathematically, it is expressed as:
\[
P \times V = \text{constant}
\]
or equivalently
\[
P = \frac{k}{V}
\]
which is essentially a power law with a negative exponent, similar to what is shown in the equation on your graph.

In your case, the fitted equation uses a power-law form with an exponent \( B \approx -1 \), which aligns with Boyle’s Law.

### Would you like further details or have any questions?

Here are some related questions to expand on this:

1. How does Boyle's Law relate to the Ideal Gas Law?
2. What are the conditions under which Boyle's Law is applicable?
3. How would changing the temperature affect the pressure-volume relationship?
4. How can we determine the amount of gas from a pressure-volume plot?
5. How would this graph change if the gas were non-ideal?

**Tip:** Remember, Boyle's Law only applies when the temperature and amount of gas remain constant during the pressure-volume changes.

Explore the pressure vs. volume relationship shown in the graph, demonstrating Boyle's Law. Learn how pressure and volume of a gas are inversely proportional and fit to a power law equation (y = A * x^B). Understand how coefficients A = 843.93 and B = -0.92683 are derived from the data.

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