A closed, adjustable cylinder containing 6.2 moles of oxygen gas has a volume of 4.3 liters and a pressure of 3.8 atmospheres. If the cylinder's volume is changed so that it is 15.5 liters, what is the new pressure of the gas? Round your answer to the nearest 0.01 atm.

The new pressure is 1.05 atm

Explanation:

Step 1: Data given

Number of moles oxygen gas = 6.2 moles

Volume of the cylinder = 4.3 L

Pressure of the gas = 3.8 atm

The volume changed to 15.5 L

Step 2: Calculate the new pressure

P1*V1 = P2*V2

⇒with P1 = the initial pressure of the gas = 3.8 atm

⇒with V1 = the initial volume = 4.3 L

⇒with V2 = the increased volume = 15.5 L

⇒with P2 = the new pressure = TO BE DETERMINED

3.8 atm * 4.3 L = 15.5 L * P2

P2 = (3.8 atm *4.3 L) / 15.5 L

P2 = 1.05 atm

The new pressure is 1.05 atm

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

може ли да зареждате повече информация, моля