The problem reads:

"A certain mass of ammonia occupies 600 ml at a certain pressure. When the pressure is changed to 4 atmospheres, it occupies a volume of 2.4 litres, temperature remaining constant. What was the initial pressure?"

Approach:

This is a problem related to Boyle's Law, which states that for a given mass of gas at constant temperature, the pressure $P$ and volume $V$ are inversely proportional: $P_1 V_1 = P_2 V_2$ Where:

• $P_1$ is the initial pressure (unknown),
• $V_1$ is the initial volume (600 ml = 0.6 L),
• $P_2 = 4 \, \text{atm}$ (new pressure),
• $V_2 = 2.4 \, \text{L}$ (new volume).

We can rearrange the formula to solve for the initial pressure $P_1$: $P_1 = \frac{P_2 V_2}{V_1}$

Calculation:

$P_1 = \frac{4 \times 2.4}{0.6} = \frac{9.6}{0.6} = 16 \, \text{atm}$

Thus, the initial pressure $P_1$ was 16 atm.

Do you want more details or have any questions?

Related questions:

1. How does Boyle's Law apply when temperature is not constant?
2. What is the effect of increasing pressure on gas volume, according to Boyle's Law?
3. How would the calculation change if the units of volume were different?
4. Can Boyle's Law be applied to all types of gases under all conditions?
5. What other gas laws are related to Boyle's Law?

Tip: Always ensure that volume and pressure units are consistent before applying gas laws like Boyle's Law.