Question

Write a balanced chemical equation based on the following description: solid yttrium metal reacts with nitrogen gas to form solid yttrium(III) nitride

Write a balanced chemical equation based on the following description: the reaction of powdered aluminum and powdered iron(III) oxide produces solid aluminum oxide and liquid iron metal

How many grams of nitric acid, \(\mathrm{HNO}_{3}\), are required to neutralize (completely react with) \(4.30 \mathrm{~g}\) of \(\mathrm{Ca}(\mathrm{OH})_{2}\) according to the acid-base reaction: \(2 \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq})\) \(\rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\)

What mass in grams of \(\mathrm{NaN}_{3}\) is required to produce \(50.2 \mathrm{~L}\) of \(\mathrm{N}_{2}\) gas (density \(=1.25 \mathrm{~g} / \mathrm{L}\) ) according to the balanced chemical reaction: 2

If you have 1 mol \(\mathrm{Xe}\) and \(1 \mathrm{~mol} \mathrm{~F}_{2}\), how many moles of \(\mathrm{XeF}_{4}\) can you create in the following chemical reaction?

Answer 1

Use mole mole relationship to problem.