A 3.20 L sample of neon at 4.57 atm is added to a 11.0 L cylinder that contains argon. If the pressure in the cylinder is 5.13 atm after the neon is added, what was the original pressure (in atm) of argon in the cylinder?
For neon gas using,
P1V1 = P2 V 2
P 1 = initial pressure of neon = 4.57 atm
V1 = initial volume = 3.2L
P2 = final pressure of neon
V2 = final volume= 11 L
Thus P2 = ( P1 V 1)/V2
P2. = (3.2L × 4.57atm)/11.0L
= 1.33 atm
Thus, the original pressure for argon gas will be = total pressure - P2
= (5.13- 1.33)atm
= 3.8 atm
A 3.20 L sample of neon at 4.57 atm is added to a 11.0 L cylinder...
A 3.20 L sample of neon at 4.57 atm is added to a 11.0 L cylinder that contains argon. If the pressure in the cylinder is 5.13 atm after the neon is added, what was the original pressure (in atm) of argon in the cylinder? I keep on gettting 5.29
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