The theoretical yield is the
yield after a certain reaction occurs. So if you are given 17.1 g of H2 and an
excess of N2, you should know the balanced equation.
N2 + 3H2 → 2NH3
Molar mass of H2 = 2.02 g/mol
Molar mass of NH3 = 17 g/mol
(17.1 g of H2)(1 mol H2/2.02g H2)(2
mol NH3/3mol H2)(17g NH3/1mol NH3) = 95.94g NH3
Answer:
<h2>
<em>Urea</em></h2>
Explanation:
<h3>
Urea = CH₄N₂O (Carbamide)</h3>
<em>It</em><em> </em><em>was</em><em> </em><em>the</em><em> </em><em>first</em><em> </em><em>organic</em><em> </em><em>compound</em><em> </em><em>to</em><em> </em><em>be</em><em> </em><em>synthesized</em><em> </em><em>in</em><em> </em><em>laboratory</em><em> </em><em>from</em><em> </em><em>the</em><em> </em><em>inorganic</em><em> </em><em>chemicals</em><em>.</em>
Thermal is the root word of heat
Answer:
Haven't evaporated all of the water
Explanation:
One of the main sources of error that occur in a formula of a hydrate lab is that all of the water is not evaporated. We can see at the end of the video that half of the CoCl2 is a light blue colors and the other half is a dark blue color. This indicates that all of the water still has not been evaporated off, resulting in the actual mass of the salt to be greater than the predicted value.