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ArbitrLikvidat [17]
3 years ago
12

Five mineral samples of equal mass of calcite, caco3 (mm 100.085) , had a total mass of 10.9 ± 0.1 g. what is the average mass o

f calcium in each sample? (assume that the relative uncertainties in atomic mass are small compared the uncertainty of the total mass.)
Chemistry
1 answer:
g100num [7]3 years ago
6 0

The molecular mass of calcite is 100.085 (given).

Atomic mass of calcium = 40.078 amu

Percent amount of calcium in calcite = \frac{40.078}{100.085}\times 100 = 40.044%

The total mass of five mineral samples = 10.9\pm 0.1 g  (given)

So, the mass of one sample = \frac{10.9}{5} = 2.18 g

and \frac{0.1}{5} = 0.02 g

The average mass of calcium in sample = \frac{2.18 g\times 40.044}{100} = 0.873 g

and \frac{0.02 g\times 40.044}{100} = 0.008 g

Hence, the average mass of calcium in each sample is 0.873 g\pm 0.008 g.

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Start with 3 breads and 2 cheeses. How many products are made? 1 What are the leftovers?
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How many particles are in 67.9 grams of water (H2O)?
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Read 2 more answers
What is the maximum mass of S8 that can be produced by combining 88.0 g of each reactant? 8SO2+16H2S⟶3S8+16H2O
Leni [432]

Answer:

124.24 g of S₈.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

8SO₂ + 16H₂S —> 3S₈ + 16H₂O

Next, we shall determine the masses of SO₂ and H₂S that reacted and the mass of S₈ produced from the balanced equation.

This is illustrated below:

Molar mass of SO₂ = 32 + (16×2)

= 32 + 32 = 64 g/mol

Mass of SO₂ from the balanced equation = 8 × 64 = 512 g

Molar mass of H₂S = (2×1) + 32

= 2 + 32 = 34 g/mol

Mass of H₂S from the balanced equation = 16 × 34 = 544 g

Molar mass of S₈ = 32 × 8 = 256 g/mol

Mass of S₈ from the balanced equation = 3 × 256 = 768 g

Thus,

From the balanced equation above,

512 g of SO₂ reacted with 544 g of H₂S to produce 768 g of S₈.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

512 g of SO₂ reacted with 544 g of H₂S.

Therefore, 88 g of SO₂ will react with = (88 × 544) / 512 = 93.5 g of H₂S.

From the calculation made above, we can see that it will take a higher mass (i.e 93.5 g) than what was given (i.e 88g) of H₂S to react completely with 88 g of SO₂.

Therefore, H₂S is the limiting reactant and SO₂ is the excess reactant.

Finally, we shall determine the maximum mass of S₈ produced from the reaction.

In this case, we shall use the limiting reactant because it will give the maximum yield of S₈ since all of it is consumed in the reaction.

The limiting reactant is H₂S and the maximum mass of S₈ produced can be obtained as follow:

From the balanced equation above,

544 g of H₂S reacted to produce 768 g of S₈.

Therefore, 88 g of H₂S will react to produce = (88 × 768) / 544 = 124.24 g of S₈.

Therefore, the maximum mass of S₈ produced from the reaction is 124.24 g.

7 0
3 years ago
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