With the combine gas law of Boyle's and Charles's law this should be easy. V1 x P1 x T2 = V2 X P2 x T1 11ml x 14.3 psi x 68 F = ? x 14.7 Psi x 59 F The new volume would be: 12.3 ml of Oxygen.
250(740)=(x)(800) x=231.25 sig. figures x=230mL
You are increasing pressure so the answer will be smaller, so multiply by 740 and divide by 800. The answer is 231.25 ml.
H
305 k
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
The volume you would expect the gas to occupy if the pressure is increased to 40 kPa would be 50 liters.
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
423mL
419 mL
Chlorine gas occupies a volume of 25 mL at 300K What volume it occupy at 600k
0.667
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
Volume = how much space an object occupies, that nothing else can occupy at the same time.
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
Volume = how much space an object occupies, that nothing else can occupy at the same time.
305 k
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
The volume is 0,046 L.