Work the entire problem from the beginning. how many grams of h2 would be formed if 34 grams of carbon reacted with an unlimited amount of h2o? the reaction is: c + h2o → co + h2 the atomic mass of c is 12.01 g/mole. the atomic mass of h2 is 2.016 g/mole. grams of hydrogen

5.66 g of would be formed if 34 grams of carbon reacted with an unlimited amount of

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number of particles.

To calculate the moles, we use the equation:

Carbon is the limiting reagent as it limits the formation of product and hydrogen is the excess reagent.

According to stoichiometry :

1 mole of carbon gives = 1 mole of

Thus 2.83 moles of carbon gives = of

Mass of

Thus 5.66 g of would be formed if 34 grams of carbon reacted with an unlimited amount of

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.