A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L? (Boyle)

Explanation:

The new pressure can be found by using the formula for Boyle's law which is

Since we are finding the new pressure

From the question we have

We have the final answer as

Hope this helps you

Given:

Initial Volume = 11.2 L

Initial Pressure = 0.860 atm

Final Volume = 15.0 L

To Find:

Final Pressure

Concept/Theory:

"At constant temperature, the pressure of a fixed amount of gas varies inversely with the volume of the gas."

It can be also stated as "At constant temperature, the product of pressure and volume of fixed amount of a gas remains constant."

If the initial pressure and volume of a fixed amount of gas at constant temperature are & and final pressure of the gas is and volume occupied is , then according to Boyle's law;

OR

By using Boyle's Law, we get:

Final Pressure = 0.642 atm

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"

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