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2 years ago

Calculate the density of chloroform

Chemistry

1 answer:

Rina8888 [55]2 years ago

5 0

Answer: The density of chloroform is 1.47 g/mL

Explanation : Given,

Volume = 40.5 mL

Mass of cylinder = 85.16 g

Mass of cylinder and liquid = 145.10 g

First we have to calculate the mass of liquid (chloroform).

Mass of liquid = Mass of cylinder and liquid - Mass of cylinder

Mass of liquid = 145.10 g - 85.6 g

Mass of liquid = 59.5 g

Now we have to calculate the density of liquid (chloroform).

Formula used:

$Density=\frac{Mass}{Volume}$

Now putting g all the given values in this formula, we get:

$Density=\frac{59.5g}{40.5mL}$

$Density=1.47g/mL$

Therefore, the density of chloroform is 1.47 g/mL

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2.56 g of hydrogen reacts completely with 20.32 g of oxygen to form X g of water. X = g

Brilliant_brown [7]

Answer:

Mass of water produced is 22.86 g.

Explanation:

Given data:

Mass of hydrogen = 2.56 g

Mass of oxygen = 20.32 g

Mass of water = ?

Solution:

Chemical equation:

2H₂ + O₂ → 2H₂O

Number of moles of oxygen:

Number of moles = mass/ molar mass

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Number of moles = mass/ molar mass

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Number of moles = 1.28 mol

Now we will compare the moles of water with oxygen and hydrogen.

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2 : 2

1.28 : 1.28

The number of moles of water produced by oxygen are less thus it will be limiting reactant.

Mass of water produced:

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Mass = 1.27 × 18 g/mol

Mass = 22.86 g

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3 years ago

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What is symbol, molecule, electrovalent compound?

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How many moles of koh are contained in 250 ml of a 2.0 m solution of koh

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Gaseous methane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 9.6 g of methane is

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Answer:

21.6 g

Explanation:

The reaction that takes place is:

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First we convert the given masses of both reactants into moles, using their respective molar masses:

9.6 g CH₄ ÷ 16 g/mol = 0.6 mol CH₄

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0.6 moles of CH₄ would react completely with (2 * 0.6) 1.2 moles of O₂. As there are more O₂ moles than required, O₂ is the reactant in excess and CH₄ is the limiting reactant.

Now we calculate how many moles of water are produced, using the number of moles of the limiting reactant:

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