The volume is approx. 15,35 litres.
What you need to know to work this out is that:- Moles of gases at standard temperature pressure (With P and T constant) are proportional to the volume they occupy, divided by their specific gas constant.
Ideal gas equation. PV = nRT ===============
The answer is 0,19 moles.
Chlorine gas occupies a volume of 25 mL at 300K What volume it occupy at 600k
the volume doubles
Approx. 774 litres.
The volume is 13,64 L.
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.
First convert the number of grams of CO2 into moles, then use the Ideal Gas Law. For how to solve this problem, see the two Related Questions links to the left of this answer.
First we need the moles of krypton gas. Monoatomic gas.0.405 grams Kr (1 mole Kr/83.80 grams)= 0.004833 moles krypton gas======================Now the ideal gas equation.PV = nRT(1 atm)(X volume) = (0.004833 moles Kr)(0.08206 L*atm/mol*K)(298.15 K)= 0.118 Liters of krypton gas--------------------------------------
1 mole of any gas at STP occupies 22.4 liters. Thus, 2 moles propane will occupy 2 x 22.4 L = 44.8 liters.
According to Avogadro's Law, the number of moles is proportional to the volume. Therefore, if the number of moles of gas decreases, the volume also decreases.
What you need to know to work this out is that:- Moles of gases at standard temperature pressure (With P and T constant) are proportional to the volume they occupy, divided by their specific gas constant.
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
Ideal gas equation. PV = nRT ===============
The answer is 0,19 moles.
3.8 kPa