Balance the following equations:
(a) \(\mathrm{Al}_{4} \mathrm{C}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{CH}_{4}(g)\)
(b) \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{2}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)
(c) \(\mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)
(d) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{MgSO}_{4}(a q)+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)\)
Text Transcription:
Al4C3(s) + H2O(l) \longrightarrow Al(OH)3(s) + CH4(g)
C5H10O2(l) + O2(g) \longrightarrow CO2(g) + H2O(g)
Fe(OH)3(s) + H2SO4(aq) \longrightarrow Fe2(SO4)3(aq) + H2O(l)
Mg3N2(s) + H2SO4(aq) \longrightarrow MgSO4(aq) + (NH4)2SO4(aq)
Step 1 of 5) A mole of any substance contains Avogadro’s number 16.02 * 10232 of formula units of that substance. The mass of a mole of atoms, molecules, or ions (the molar mass) equals the formula weight of that material expressed in grams. The mass of 1 molecule of H2O, for example, is 18.0 amu, so the mass of 1 mol of H2O is 18.0 g. That is, the molar mass of H2O is 18.0 g>mol.The empirical formula of any substance can be determined from its percent composition by calculating the relative number of moles of each atom in 100 g of the substance. If the substance is molecular in nature, its molecular formula can be determined from the empirical formula if the molecular weight is also known. Combustion analysis is a special technique for determining the empirical formulas of compounds containing only carbon, hydrogen, and/or oxygen.The mole concept can be used to calculate the relative quantities of reactants and products in chemical reactions. The coefficients in a balanced equation give the relative numbers of moles of the reactants and products. To calculate the number of grams of a product from the number of grams of a reactant, first convert grams of reactant to moles of reactant. Then use the coefficients in the balanced equation to convert the number of moles of reactant to moles of product. Finally, convert moles of product to grams of product.
