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Doss [256]
2 years ago
6

6. The reaction of quicklime, CaO, with water produces slaked lime, Ca(OH)2, which is widely used in the construction industry t

o make mortar and plaster. The reaction of quicklime and water is highly exothermic: CaO(s) + H2 O(l) ⟶ Ca(OH)2(s) ΔH = −350 kJ mol−1
Chemistry
1 answer:
vlabodo [156]2 years ago
5 0

Answer:

1) Enthalpy of reaction per gram of quick lime or calcium oxide is -6.25 kJ/g.

2)4.730\times 10^6kilo Joules of energy is produced when 1 Tonn of slaked lime is produced.

Explanation:

CaO(s) + H_2O(l)\rightarrow Ca(OH)_2(s),\Delta H=-350 kJ/mol

Enthalpy of reaction = ΔH = -350 kJ/mol

1 mole of calcium oxide = 56 g/mol

1 ) Enthalpy of reaction per gram of quick lime or calcium oxide:

\frac{\Delta H}{56 g/mol}=\frac{-350 kJ/mol}{56 g/mol}=-6.25 kJ/g

2) Mass of slake lime = 1 Tonn = 1,000,000 g

Moles of slaked lime = \frac{1,000,000}{74 g/mol}=13,513.51 mol

According to reaction, on formation of 1 mol of slaked lime 350 kilo Joules of energy is produced.

Then energy produced when 13,513.51 moles of slaked lime is produced:

350 kJ\times 13,513.51 =4.730\times 10^6 kJ

4.730\times 10^6kilo Joules of energy is produced when 1 Tonn of slaked lime is produced.

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Valentin [98]

Answer:

0.54 mole of H2O.

Explanation:

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

2CH3OH + 3O2 —> 2CO2 + 4H2O

From the balanced equation above,

2 moles of CH3OH reacted to produce 4 moles of water.

Finally, we shall determine the number of mole of water (H2O) produced by the reaction of 0.27 moles of CH3OH. This can be obtained as follow:

From the balanced equation above,

2 moles of CH3OH reacted to produce 4 moles of water.

Therefore, 0.27 moles of CH3OH will react to produce = (0.27 × 4)/2 = 0.54 mole of H2O.

Thus, 0.54 mole of H2O is produced from the reaction.

5 0
2 years ago
450.0 mL of an unknown gas has its pressure decreased from 0.07 atm to 0.04 atm. Assuming temperature remains constant, what wou
tino4ka555 [31]

The final volume of the unknown gas is 787.5 ml

Given:

volume of unknown gas = 450.0 mL

initial pressure of unknown gas = 0.07 atm

final pressure of unknown gas = 0.04 atm

To Find:

final volume of the unknown gas

Solution:

Substituting these values into Boyle’s law, we get

P1V1 = P2V2

(0.07)(450) = (0.04)V2

V2 = (0.07)(450)/(0.04)

V2 = 787.5

So, final volume of the unknown gas is 787.5 ml

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4 0
2 years ago
If the results of an experiment disprove a hypothesis, then the a. results should not be reported. b. hypothesis is just a theor
Alina [70]
B.Hypothesis is just a theory.
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2 years ago
How many moles of hydrogen gas will be produced when 12 g of Mg will react completely with excess of an acid according to the fo
lina2011 [118]

Answer:

0.49 mol

Explanation:

Step 1: Write the balanced equation

Mg + 2 HCI ⇒ MgCl₂ + H₂

Step 2: Calculate the moles corresponding to 12 g of Mg

The molar mass of Mg is 24.31 g/mol.

12g \times \frac{1mol}{24.31g} = 0.49mol

Step 3: Calculate the moles of H₂ produced by 0.49 moles of Mg

The molar ratio of Mg to H₂ is 1:1. The moles of H₂ produced are 1/1 × 0.49 mol = 0.49 mol.

7 0
3 years ago
Describe the ways in which ionic compound nomenclature differs from covalent compound nomenclature
Igoryamba

Answer:

Ionic compound are when electrons are given to another element, making one atom positive and the other negative, so they attract. Covalent compound is when both atoms share electrons with each other.

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3 years ago
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