Question

a flask containg 2.7 of hydrogen was collceted under a pressure of a 4.5 atm. what preussre would havw bewn reqired for the voulme of the gas to have been 7.2 L ( assuming a constant temperture)

Answer 1

Explanation: Step 1: Identify the given information We are given the following information: - Initial volume (V1) = 2.7 L - Initial pressure (P1) = 4.5 atm - Final volume (V2) = 7.2 L - Final pressure (P2) = ? Step 2: Use Boyle's Law Boyle's Law states that the pressure of a gas is inversely proportional to its volume, as long as the temperature and the amount of gas remain constant. Mathematically, it can be represented as: P1 * V1 = P2 * V2 Step 3: Solve for the final pressure (P2) We can rearrange the equation to solve for P2: P2 = (P1 * V1) / V2 Now, plug in the given values: P2 = (4.5 atm * 2.7 L) / 7.2 L P2 = 12.15 / 7.2 P2 ≈ 1.6875 atm Step 4: Round the answer Since we are dealing with pressure, it is common to round the answer to two decimal places: P2 ≈ 1.69 atm