How many liters of Hydrogen gas are formed from the complete reaction of 1.07 moles of carbon. C h20--- CO H2?

Answer 1

You stated the amount of carbon you had, but how much water (separated into its constituents by electrolysis, otherwise if you dump water on carbon you wind up with nothing more than wet carbon) is available? Let's assume you've got an excess of it and go from there.

In a real-life situation you won't get any hydrogen gas. In order of reactivity are hydrogen, oxygen and carbon. One of three things will happen here.

The most likely reaction is that the hydrogen and oxygen will recombine into water and, once again, you've got wet carbon...that is, unless the heat from the very exothermic 2H2 + O2 -> 2H2O reaction sets the carbon on fire, in which case it'll scavenge atmospheric O2 and you'll receive some CO2, some CO and a little free carbon, aka "soot."

Under different circumstances, you might get some CH4 and some O2. And because you have 1.07 moles C, you'll wind up with 1.07 moles methane - giving you 23.968 liters of methane at STP.

If you have a really nice lab that can emulate photosynthesis, you could convert the three elements into glucose. That's not too likely; you will probably wind up with the same block of carbon and glass of water that you started out with.

The chemical reaction should be written as shown below :

C + H2O -----> CO + H2

The balanced chemical reaction equation indicates that 1.0 mole of H2 gas is produced for each mole of carbon that reacts. Therefore you have :

n H2 = (1.07 mole C ) ( 1.0 mole H2 / 1.0 mole C ) = 1.07 moles H2

At STP, there are 22.7 L per mole of ideal gas. Therefore the H2 liters at STP is given by :

V H2 at STP = ( 22.7 L at STP / mole ideal gas ) ( 1.07 moles H2 )

V H2 at STP = 24.3 L of H2 at STP <-------------------------

Answer 2

The chemical reaction should be written as shown below :

C + H2O -----> CO + H2

The balanced chemical reaction equation indicates that 1.0 mole of H2 gas is produced for each mole of carbon that reacts. Therefore you have :

n H2 = (1.07 mole C ) ( 1.0 mole H2 / 1.0 mole C ) = 1.07 moles H2

At STP, there are 22.7 L per mole of ideal gas. Therefore the H2 liters at STP is given by :

V H2 at STP = ( 22.7 L at STP / mole ideal gas ) ( 1.07 moles H2 )

V H2 at STP = 24.3 L of H2 at STP <-------------------------