How do you balance $AlBr_3 + K_2SO_4 -> KBr + Al_2(SO_4)_3$?

In the one mole of $Al_2(CO_3)_3$ there are $N_A$ formula units, i.e. $6.022xx10^23$ formula units. $"Moles of aluminum carbonate"$ $=$ $"Mass"/"Molar mass"$ $=$ $(47.6*g)/(233.99*g*mol^-1)$ $=$ $0.203*mol$ But in each...

The first thing that you need to do here is to convert the mass of aluminium carbonate to moles by using the compound's molar mass. In this case, you...

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...

$"Aluminum"$ typically forms $Al^(3+)$ ions; given that we know that sulfate forms a $SO_4^(2-)$ the of the salt is clear.

Putting 3 as cooefficient for sulfur trioxide will balance the chemical equation. Check the number of atoms of each element by having an inventory. Reactant Side: $Al=2xx1=2$ $S=3xx1xx1=3$ $O=3xx4xx1=12$ Product...

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...

Is this equation balanced? How do you know? All I have done here is practise $"stoichiometry"$, and ensured $"garbage out"="garbage in"$.

$AlBr_3(s) + 3K(s) rarr Al(s) + 3KBr(s)$ This is actually a redox reaction; however, it does illustrate the required . The given reaction is certainly balanced with respect to mass...

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...

Balanced Equation $"3Ba + Al"_2"(SO"_4)_3"$$rarr$$"2Al + 3BaSO"_4$ The coefficients are the moles of each substance, and they can be used as molar ratios between two of the substances. No coefficient...