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The volume of ammonia gas at 1.09 atm of pressure is gradually decreased from 80.8 mL to 35.9 mL. What is the final pressure of ammonia if there is no change in temperature?

Answer :

Final answer:

Using Boyle's law, which states that at constant temperature, the pressure and volume of a gas are inversely proportional, we can calculate that the final pressure of the ammonia gas, when its volume is decreased from 80.8 mL to 35.9 mL, is approximately 2.46 atm.

Explanation:

The principle that applies here is the Boyle's law, which states that if the temperature remains constant, the volume of a given amount of gas is inversely proportional to the pressure. Thus, as volume decreases, the pressure increases, and vice versa.

According to the formula for Boyle's law (P1V1 = P2V2), we can find the final pressure. Given P1 (initial pressure) is 1.09 atm, V1 (initial volume) is 80.8 mL, and V2 (final volume) is 35.9 mL.

To find P2 (final pressure), we rearrange the equation: P2 = P1V1/V2. Substituting in the given values, we get: P2 = 1.09 atm * 80.8 mL / 35.9 mL. Therefore, the final pressure of the ammonia gas, when the volume is reduced and the temperature remains the same, is approximately 2.46 atm.

Learn more about Boyle's law here:

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