How many moles of oxygen gas are there in 11.2 liters at atmosphere and pressure and 546 degrees kelvin?

For propane we have 3 carbons and 8 hydrogen atoms, so the gram-molecular weight is (312 + 81) = 44g/mol. The mole ratio of oxygen to carbon dioxide is 5:3,...

The final pressure will double as well. If you use the equation, $PV = nRT$, to express the initial and the final states of your gas sample, you can...

This is an example of which states that the volume of a gas varies inversely with pressure, when mass and temperature are kept constant. Equation $V_1P_1=V_2P_2$, where $V$ is volume...

...according to the combined gas equation... We solve for....$V_2=(P_1V_1)/T_1xxT_2/P_2$ $=(150*kPaxx200*L)/(273*K)xx(546*K)/(600*kPa)=??*L$

Since the gas it is getting compressed with a change on temperature, we consider that the pressure is constant, and of course the number of mole is constant (same gas),...

Data:- Initial Volume$=V_1=60 liter$ Initial Temperature$=T_1=546K$ Final Temperature$=T_2=273K$ Final Vloume$=V_2=??$ Sol:- Since the pressure is constant and the question is asking about temperature and volume, i.e, $V_1/T_1=V_2/T_2$ $implies V_2=(V_1*T_2)/T_1=(60*273)/546=60/2=30liter$ $implies...

This means that for $6mol$ of $FeO$, only $3mol O_2$ is produced (half the moles). The volume of the oxygen is dependant on temperature and pressure. E.g. : If...

Start by using the ideal gas equation to figure out the the number of moles $O_2$ used. $ P*V= n*R*T$ Where $P" "$ is the pressure expressed in atm. $V"...

The idea here is that the of each gas will be proportional to the mole fraction each gas has in the mixture $->$ think Dalton's Law of Partial Pressures....

You'd use , which links an ideal gas' volume to its temperature if pressure and number of moles are kept constant. The mathematical formula is this $V_1/T_1 = V_2/T_2$...