The volume of a sample of oxygen is 300.0 mL, when the pressure is 1.00 atm and the temperature is 300K. At what pressure will the volume be 1000.0 mL and a temperature of 500K?

The new pressure is 0.5 atm

Explanation:

Step 1: Data given

Volume of oxygen = 300 mL = 0.300 L

Pressure = 1.00 atm

Temperature = 300 K

The volume increases to 1000mL = 1.00 L

The temperature increases to 500 K

Step 2: Calculate the new pressure

(P1*V1)/T1 = (P2*V2)/T2

⇒with P1 = the initial pressure = 1.00 atm

⇒with V1 = the initial volume = 0.300 L

⇒with T1 = the initial temperature = 300 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with V2 = the increased volume = 1.00 L

⇒with T2 = the increased temperature = 500 K

(1.00 atm* 0.300 L)/300 K = (P2 * 1.00L) / 500 K

P2 = (1.00 *0.300 * 500) / (300 *1.00)

P2 = 0.5 atm

The new pressure is 0.5 atm

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.