In the following reaction, eight moles of sodium hydroxide is broken down into four moles of sodium oxide and four moles of wate
1 answer:
Answer:
21.344%
Explanation:
For the given chemical reaction, 8 moles of the reactant should produce 4 moles of . However, 195 g of
was produced instead. The molar mass of
is 61.9789 g/mol.
Thus, the moles of produced = 195/61.9789 = 3.1462 moles
The percent error = [(Actual -Experiment)/Actual]*100%
The percent error = [(4.00 - 3.1462)/4.00]*100% = (0.85376/4.00)*100% = 21.344%
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Answer:
a) No molecules of hydrogen
b) four molecules of ammonia
c) four left molecules of nitrogen.
Explanation:
The balanced reaction between nitrogen and hydrogen molecules to give ammonia molecules is:
Thus one molecule of nitrogen will react with three molecules of hydrogen to give two molecules of ammonia.
We have six molecules of each nitrogen and hydrogen in the closed container and they undergo complete reaction it means the limiting reagent is hydrogen. For six molecules of nitrogen, eighteen molecules of hydrogen will be required.
So six molecules of hydrogen will react with two molecules of nitrogen to give four molecules of ammonia.
The product mixture will have
a) No molecules of hydrogen
b) four molecules of ammonia
c) four left molecules of nitrogen.