0
What volume of oxygen gas at 320k and 680 torr will react with 2.50 L?
Wiki User
∙ 14y agoWant this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
P1V1 = P2V2 (740 torr)(500 ml) = (780 torr)V2 V2 = (740 torr)(500 ml) / (780 torr) V2 ~ 474 ml
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
P1*V1 = P2*V2, Therefore your numerical answer would be 100*810/72 torr.
A 37.7 ml volume of an unknown gas is collected over water at 19 degrees celsius and a total pressure of 770 torr The mass of the gas is 68.6 mg What volume does the gas occupy?
the gas occupies a volume of37.7 ml as stated in the question either your question is wrong or incomplete.
a gas has a pressure of 766.7 torr at a temperature of 10.0°C. the sample contains 2.35 moles of xenon. what is the volume of the gas in liters?
Using PV=nRT, 10.0ºC = 283.15ºK, R = 62.36 L torr/mol K V= (nRT)/P V = (2.35m*(62.36 L torr/mol K)*283.15ºK)/766.7 Torr V = 54.12 L
What is the partial pressure of N2 and O2 having a total pressure of 1075 torr if the partial pressure of 02 is 720 torr?
1075 torr - 720 torr = 355 torr
A 125.0 mL sample of nitrogen at 790 torr was compressed to a volume of 75.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1300<--- torr
What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
P1V1 = P2V2 (740 torr)(500 ml) = (780 torr)V2 V2 = (740 torr)(500 ml) / (780 torr) V2 ~ 474 ml
A 110.0 mL sample of nitrogen at 820 torr was compressed to a volume of 83.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
A 100.0 mL sample of nitrogen at 810 torr was compressed to a volume of 72.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
How to convert percent oxygen into pO2 Torr?
transver it though diffrent containers
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
P1*V1 = P2*V2, Therefore your numerical answer would be 100*810/72 torr.
What pressure is needed to compress the air in a 1.105 liter cylinder at 755 torr to a volume of 1.00 ml?
p1.V1 = p2.V2 (Boile-GayLussac's gas law) 755(torr)*1105(mL) = p2(torr)*1.00(mL) The pressure is 755*1105= 8.34*105 torr = 1098 atm. (which looks rather high to me for practical purposes, and maybe oxygen / nitrogen become fluidised; moreover is your cylinder designed for pressure over -safety!- 3000 atm??)
Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22C and 100 kPa?
The ideal gas equation.PV = nRT22o C = 295.15 Kelvin(750 Torr)(X volume) = (1.5 moles O2)(62.36 L*torr/mol*K)(295.15 K)Volume = 27608.331/750= 37 Liters oxygen gas=================
What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure is 39,8 torr.
The gases in a mixture have the following partial pressures at the same volume and temperature 1013000 Pa nitrogen 700 mm argon 1.20 ATM of helium 790 torr oxygen and 0.50 ATM of carbon dioxide?
Carbon dioxide Argon Oxygen Helium Nitrogen
A sample of propane a component of LP gas has a volume of 35.3 L at 315 K and 922 torr What is its volume at STP?
37.1L is the answer
