Samples with masses of 5.5 g 2.27 g and 0.8995 g are mixed together. The sum of the masses of the three
1 answer:
Answer:
Explanation:
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In this case, it is widely known that when measurements with different significant figures are put under mathematical operations, the final result must be displayed with the same amount of significant figures of the shortest measurement, thus, due to the fact that 5.5 g has two significant figures only the result is consequently shown with two significant figures as well as shown down below:
By rounding the first six to seven due to the fact that the next six is greater than five, according to rounding rules, the result is:
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Answer:
The percent yield of a reaction is 48.05%.
Explanation:
Volume of water obtained from the reaction , V= 5.76 mL
Mass of water = m = Experimental yield of water
Density of water = d = 1.00 g/mL
Theoretical yield of water : T
Moles of tungsten(VI) oxide =
According to recation 1 mole of tungsten(VI) oxide gives 3 moles of water, then 0.2220 moles of tungsten(VI) oxide will give:
Mass of 0.6660 moles of water:
0.666 mol × 18 g/mol = 11.988 g
Theoretical yield of water : T = 11.988 g
To calculate the percentage yield of reaction , we use the equation:
The percent yield of a reaction is 48.05%.