Solve Trapped Gas Chemistry Help Please?
Chemistry help please? - solve trapped gas
The pressure of a sample of helium in a container of 1.74 L is 0.988 atm. What is the pressure again when the sample is placed in a vat of 2.53 L?
The use of Gay-Lussac, in order to solve this puzzle. P1 = 128 kPa, T1 = 269 K, T2 = 369 K, P2 =?
What volume of 1.01 moles of carbon monoxide in normal operation?
The trapped air in a cylinder with a piston is located to 123.3 ml of 1.08 bar pressure. What is the new volume of air when the pressure increases to 1.35 ATM with the force of the piston?
An air sample into a syringe exerts a pressure of 1.17 bar at a temperature of 23.0 ° C. The syringe will be included in a boiling water bath at 100.0 ° C. The atmospheric pressure is greater than 1.25 bar pressure, the piston, reducing the volume of 0231 ml What was the volume of air originally?
The pressure on a sample of 240.9 ml of helium increases from 0.415 atm to 1.43 ATM. What is the new band, under the assumption of constant temperature?
|
2 comments:
Gas ...
New 67,949 atm pressure (Boyle's Law)
175.58 kPa (P / T = P / T)
1.01 mol CO employ 22,624 liters.
98.64 ml 4 for the number
195 ml of # 5 (Combined Gas Law PV / T = PV / T
69.9 ml of the Law on the last (re Boyle)
Make your own freaking homework! These are the equations of the simple volume printing ... Simply connect the data and solve!
Post a Comment