A gas has an initial volume of 2.4 L at a pressure of 1.5 atm and a temperature of 273 K. The pressure of the gas increases to 4.5 atm, and the temperature of the gas increases to 313 K. What is the final volume of the gas? 0.70 L 0.92 L 6.3 L 8.3 L

Final volume of the gas v2 = 0.92 L (Approx.)

Explanation:

Given:

Initial volume v1 = 2.4 L

Pressure p1 = 1.5 atm

Temperature t1 = 273 K

New pressure p2 4.5 atm

New temperature t2 = 313 K

Find:

Final volume of the gas v2

Computation:

p1v1 / t1 = p2v2 / t2

(1.5)(2.4) / 273 = (4.5)(v2) / 313

v2 = 0.9172

Final volume of the gas v2 = 0.92 L (Approx.)

hloride, what is the mass of calcium in

explanation:

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.