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zheka24 [161]
3 years ago
15

Calculate the amount of CO2 (in kg) released when 1 kg of coal is burned. Assume that carbon content of the coal is 50% by mass.

Chemistry
1 answer:
Delvig [45]3 years ago
4 0

Answer:

1.8321 kg

Explanation:

The given 1 kg of coal contains 50% of the carbon atom by mass. Thus, mass of carbon in coal is \frac {50}{100}\times 1\ kg=0.5\ kg

Also, 1 kg = 1000 g

So, mass of carbon = 500 g

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Molar mass of carbon = 12.0107 g/mol

Moles of methanol = 500 g / 12.0107 g/mol = 41.6295 moles

Considering the reaction:

C+O_2\rightarrow CO_2

From the reaction,

1 mole of C react to form 1 mole of CO_2

So,

41.6295 moles of C react to form 41.6295 moles of CO_2

Moles of CO_2 = 41.6295 moles

Molar mass of CO_2 = 44.01 g/mol

So, Mass = Moles × Molar mass = 41.6295 moles × 44.01 g/mol = 1832.1143 g

Also, 1g = 0.001 kg

<u>So, amount of CO_2 released = 1.8321 kg</u>

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If 30 grams of KCl is dissolved at 10°C, how many additional grams would be needed to make the solution saturated at 60°C? * Cap
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If 30 grams of KCl is dissolved at 10°C, 14 g of KCl should be added to make a saturated solution at 60 °C.

<h3>What is a saturated solution?</h3>

A saturated solution is a solution in which there is so much solute that if there was any more, it would not dissolve. Its concentration is the same as the solubility at that temperature.

  • Step 1. Calculate the mass of water.

At 10 °C, the solubility is 31.2 g KCl/100 g H₂O.

30 g KCl × 100 g H₂O/31.2 g KCl = 96 g H₂O

  • Step 2. Calculate the mass of KCl required to prepare a saturated solution at 60 °C.

At 60 °C, the solubility is 45.8 g KCl/100 g H₂O.

96 g H₂O × 45.8 g KCl/100 g H₂O = 44 g KCl

  • Step 3. Calculate the mass of KCl that must be added.

44 g - 30 g = 14 g

If 30 grams of KCl is dissolved at 10°C, 14 g of KCl should be added to make a saturated solution at 60 °C.

Learn more about saturated solutions here: brainly.com/question/24564260

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