2H2 + O2 → 2H2O
First, we will find the moles :
n H2 = m H2 / Mr H2
n H2 = 10 / 2
n H2 = 5 mole
n O2 = m O2 / Mr O2
n O2 = 5 / 16
n O2 = 0.3125 mole
n H2 / coef. H2 > n O2 / coef. O2
So, O2 is the limiting reactant
The mass of water produced :
n H2O = (coef. H2O / coef. O2) • n O2
n H2O = (2/1) • 0.3125
n H2O = 0.625 mole
m H2O = n H2O • Mr H2O
m H2O = 0.625 • 18
m H2O = 11.25 gr
Excesses reactant :
n H2 = 5 - 0.625 = 4.375 mole
m H2 = n H2 • Mr H2
m H2 = 4.375 • 2
m H2 = 8.75 gr
Answer:
the picture above should help you
<span>Endothermic reactions take in heat from the environment in order to react while exothermic reactions release heat during the reaction. For this, D must be true as the products have less energy because they have released heat during the reaction. A and C are incorrect because they products and reactants are equal and B is wrong because the energy of the products would be more as the reaction took in heat.</span>
