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sleet_krkn [62]
3 years ago
15

Battery acid has a density of 1.285 g/mL and contains 38.0% sulfuric acid by mass. The car battery contains 1.45 L of battery ac

id. What is the mass of the sulfuric acid in a car battery?
Chemistry
1 answer:
larisa86 [58]3 years ago
5 0

Answer: 708.2 grams

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

Given : 38 g of H_2SO_4 is dissolved in 100 g of solution.

Density of solution = 1.285 g/ml

Volume of solution = \frac{mass}{density}=\frac{100g}{1.285g/ml}=77.8ml

Thus if 77.8 ml of H_2SO_4 contains = 38 g of H_2SO_4

1.45L= 1450 ml of H_2SO_4 contains = \frac{38}{77.8}\times 1450=708.2 g of H_2SO_4

Therefore, the mass of the sulfuric acid in a car battery is 708.2 g

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Calculate the mass, in grams, of Ag2CrO4 that will precipitate when 50.0mL of 0.20M AgNO3 solution is mixed with 40.0mL of 0.10M
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Answer:

1.327 g Ag₂CrO₄

Explanation:

The reaction that takes place is:

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First we need to <em>identify the limiting reactant</em>:

We have:

  • 0.20 M * 50.0 mL = 10 mmol of AgNO₃
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If 4 mmol of K₂CrO₄ were to react completely, it would require (4*2) 8 mmol of AgNO₃. There's more than 8 mmol of AgNO₃ so AgNO₃ is the excess reactant. <em><u>That makes K₂CrO₄ the limiting reactant</u></em>.

Now we <u>calculate the mass of Ag₂CrO₄ formed</u>, using the <em>limiting reactant</em>:

  • 4 mmol K₂CrO₄ * \frac{1mmolAg_2CrO_4}{1mmolK_2CrO_4} *\frac{331.73mg}{1mmolAg_2CrO_4} = 1326.92 mg Ag₂CrO₄
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2 years ago
If a scientist knows the relative age of a fossil, he can also know
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The ratio O/Fe is:

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<h3>Fe₂O₃</h3>
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