How many moles of H2O could be obtained by reacting 0.75 mole of H2O2 in the reaction H2O2+H2S→2H2O+S?

Question

Mateo Aguilar · Accepted Answer

1.5 moles of water could be obtained.

The balanced chemical equation is the first thing we should always aim for since it indicates the ratios in which the reactants will react and the amount of product that will be produced. #H_2O_2+H_2Srarr2H_2O+S# This equation tells us that for every mole of #H_2O_2#, two moles of water are produced. Therefore: #n(H_2O)=2*n(H_2O_2)=2*0.75=1.5" "mol#

Luna Chen · Answer

#"1.5 mol H"_2"O"#

Balanced Equation

#"H"_2"O"_2 + "H"_2"S"##rarr##"2H"_2"O" + "S"#

Multiply the given mol #"H"_2"O"# by the mole ratio between #"H"_2"O"# and #"H"_2"O"_2#.

#0.75color(red)cancel(color(black)("mol H"_2"O"_2))xx(2"mol H"_2"O")/(1color(red)cancel(color(black)("mol H"_2"O"_2)))="1.5 mol H"_2"O"#

You can reason out the answer without having to do the math. Notice by looking at the balanced equation, that for every one mole of #"H"_2"O"_2"# in the reactants, there are two moles #"H"_2"O"# in the products. So any number of moles of #"H"_2"O"_2"# will produce twice as many moles of #"H"_2"O"#.

Luna Chen · Answer

What does the stoichiometry say..........? It says that #1*mol# of hydrogen peroxide and #1*mol# hydrogen sulfide gives #2 *mol# of water and #1*mol# of sulfur.

The stoichiometric reaction is present: #H_2O_2(l) + H_2S(g) rarr 2H_2O(l) + S(s)darr# Is it balanced? For every reactant particle is there a corresponding product particle? There must be if the reaction represents chemical reality. It is balanced, and you have done the work not me. The reaction tells me UNEQUIVOCALLY that #34*g# of hydrogen peroxide reacts with #34*g# hydrogen sulfide to give #36*g# water and #32*g# sulfur. All of these masses correspond to molar equivalents. Charge and mass are balanced as required. From where did I get these masses? Did I just look them up? Your starting conditions propose that #0.75*mol# hydrogen peroxide reacts, to give, THEREFORE, #27*g# #H_2O#, and #24*g# sulfur. Do you agree? This is an important principle to master, and if you don't from where we are coming, ask again. And note that #0.75*mol# #H_2O_2# represents a mass of #0.75*molxx34*g*mol^-1-=25.5*g#........etc........

Cameron Andrews · Answer

undefined 0.75 moles of H₂O₂ would produce 0.75 moles of H₂O in the given reaction.