The following chemical equation is not balanced: $Fe_2O_3 + H_2SO_4 -> Fe_2(SO_4)_3 + H_2O$. When this chemical equation is correctly balanced, what is the coefficient of the water molecule?

Here, we use as we would use any other collective number: a dozen eggs; a Bakers' dozen; a Botany Bay dozen. Of course, the mole specifies a much larger quantity,...

Sulfuric acid donates 2 equiv of $H_3O^+$ to aqueous solution. $H_2SO_4 + H_2O rarr HSO_4^(-) + H_3O^+$ $HSO_4^(-) + H_2O rarr SO_4^(2-) + H_3O^+$ The first equilibrium lies almost quantitatively...

It is given that both salts contain the same number of sulfur atoms. Thus we have $Al_2S_3O_12$, and necessarily $3$ $xx$ $H_2SO_4$. There are $3$ $"equiv"$ sulfuric acid per equiv...

Let's eliminate unknowns backwards, starting with $G$. From the equations for $H$, $Mn$, $K$ and $Fe$ we find: $G=C$ $F=B$ $E=1/2 B$ $D=1/2 A$ Substituting these in the...

Start by looking at the most complex compound, and balancing around that. In this case, its $Fe_2(SO_4)_(3(aq))$. We see that we need 2 Fe and 3 $SO_4$ on the...

$H_2SO_4 + B(OH)_3 → B_2(SO_4)_3 + H_2O$ We have: LHS H= 2 + 3= 5 S= 1 B= 1 O= 4 + 3= 7 RHS H= 2 S= 3 B=2...

$2$ $Al(s)$ + $3$ $H_2SO_4(aq) to $ $Al_2(SO_4)_3(aq)$ + $3$ $H_2(g)$ First calculate the number of moles of $Al$ in $7.25$ $g$, knowing the molar mass of $Al$ is $27$...

Since aluminium sulphate is in excess, it implies that sodium hydroxide is the limiting reactant and decides how much product is formed as it gets used up first. The balanced...

$HCl(aq)+H_2O(l)rarr Cu^(2+) + 2NO_3^-$ $Ca(OH)_2(s) stackrel(H_2O)rarr Ca^(2+) +2HO^-$ $Ca(NO_3)_2(s) stackrel(H_2O)rarr Ca^(2+) +2NO_3^-$ $NH_3(aq) +H_2O(l) rightleftharpoonsNH_4^+ + HO^-$ And one of these things is not like the other ones.........

An acid is a proton donor; a base is a proton acceptor. are substances that respectively increase concentrations of the characteristic cation and the characteristic anion of the ,...