A gas occupying a volume of of 725mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?
2006-08-28 22:20:50 · 8 answers · asked by Lorenz 2 in Science & Mathematics ➔ Chemistry
Initial Volume,V1 = 725 mL
Initial Pressure, P1 = 0.97 atm
Final Volume, V2 = ?
Final Pressure, P2 = 0.541 atm
Charles Law can be applied
i.e., V1P1 = V2P2
V2 = V1P1 / P2
V2 = 725 x 0.97 / 0.541
V2 = 1299.91 (approx.) mL
Therefore Final Volume of the gas is 1299.91 mL
2006-08-28 22:27:36 · answer #1 · answered by Anonymous · 1⤊ 1⤋
1300mL
Boyles law:
P1V1 = P2V2
V2 = P1V1/P2
= 725 X 0.97 / 0.541= 1299.9 = 1300mL
2006-08-28 22:29:35 · answer #2 · answered by SAREK 3 · 1⤊ 0⤋
Look on uer notebook, you will find the solution easily
2006-08-28 23:37:53 · answer #3 · answered by basimsaleh 4 · 0⤊ 1⤋
With proper rounding the correct answer is...
1299.908mL
Boyles law is extremely intuitive!
2006-08-28 22:42:47 · answer #4 · answered by TrickMeNicely 4 · 0⤊ 1⤋
The answer is:V2=1299.907ml
2006-08-28 23:57:01 · answer #5 · answered by Silent_princes 1 · 0⤊ 1⤋
use the ideal gas law equation instead of having others do your homework, you should know this, how are you going to do this on your test?
2006-08-28 22:32:35 · answer #6 · answered by Anonymous · 0⤊ 3⤋
man do it ya self its really easy
i no u cud do it
2006-08-28 22:33:36 · answer #7 · answered by Anonymous · 0⤊ 1⤋
men''''' do it urself its really simple
2006-08-28 22:55:09 · answer #8 · answered by Anonymous · 0⤊ 1⤋