Questions: Question 4 8 pts 1) A student using 5.25 L of hydrogen gas at 3.01 atm determines that its pressure decreases to 2.88 atm over the span of thirty minutes. At what volume, in mL, did the gas expand? Record your answer to tenths place and include a proper unit. (5 pts.) 2) Explain the relationship observed between the data recorded by the student below. (3 pts.) Volume and Pressure of a Gas Sample Volume (mL) Pressure (atm) 1200 0.5 600 1.0 300 2.0 150 4.0 100 6.0

Solution Steps

We need to determine the new volume of hydrogen gas when its pressure decreases from 3.01 atm to 2.88 atm. The initial volume is given as 5.25 L. We will use Boyle's Law, which states that for a given mass of gas at constant temperature, the product of pressure and volume is constant: \( P_1 V_1 = P_2 V_2 \).

Given:

• Initial pressure, \( P_1 = 3.01 \, \text{atm} \)
• Initial volume, \( V_1 = 5.25 \, \text{L} \)
• Final pressure, \( P_2 = 2.88 \, \text{atm} \)

We need to find the final volume, \( V_2 \).

Using Boyle's Law: \[ P_1 V_1 = P_2 V_2 \]

Substitute the known values: \[ 3.01 \times 5.25 = 2.88 \times V_2 \]

Rearrange the equation to solve for \( V_2 \): \[ V_2 = \frac{3.01 \times 5.25}{2.88} \]

Calculate \( V_2 \): \[ V_2 = \frac{15.8025}{2.88} \approx 5.4865 \, \text{L} \]

Convert the volume from liters to milliliters (1 L = 1000 mL): \[ V_2 = 5.4865 \times 1000 = 5486.5 \, \text{mL} \]

The data provided in the table shows an inverse relationship between volume and pressure, which is consistent with Boyle's Law. As the volume decreases, the pressure increases, and vice versa. This is because the product of pressure and volume remains constant for a given amount of gas at constant temperature.

Final Answer