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3 years ago

What do you call each of the following changes of state:

Chemistry

1 answer:

Alinara [238K]3 years ago

8 0

a. Solid to liquid - melting process

b. Liquid to gas - evaporation process

c. Gas to solid - deposition process

d. Solid to gas - sublimation process

e. Liquid to solid - solidification process

f. Gas to liquid - condensation process

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What is the minimum mass of magnetite (Fe,O2), a iron ore, from which 120. g of pure iron could be extracted? Be sure your answe

Schach [20]

Answer:

166 g

Explanation:

Step 1: Write the reaction for the obtaining of Fe from magnetite

Fe₃O₄ ⇒ 3 Fe + 2 O₂

Step 2: Calculate the moles corresponding to 120 g of Fe

The molar mass of Fe is 55.85 g/mol.

120 g × (1 mol/55.85 g) = 2.15 mol

Step 3: Calculate the moles of Fe₃O₄ required to produce 2.15 moles of Fe

The molar ratio of Fe₃O₄ to Fe is 1:3. The moles of Fe₃O₄ required are 1/3 × 2.15 mol = 0.717 mol

Step 4: Calculate the mass corresponding to 0.717 moles of Fe₃O₄

The molar mass of Fe₃O₄ is 231.53 g/mol.

0.717 mol × 231.53 g/mol = 166 g

6 0

3 years ago

AP CHEM answer and i will give brainliest, image attached

scoundrel [369]

Answer:

what is this i dont know what kind of math this is

6 0

2 years ago

4 moles of hydrogen react with 5 moles of oxygen to form water, identify the excess reagent?

Fynjy0 [20]

Answer:

Excess Reagent = oxygen

Explanation:

Limiting reagent: The substance that is totally consumed when the reaction is completed.

Excess reagent: The substance left after the limiting reagent is consumed completely

The balanced chemical equation for formation of water is as follow:

$2H_{2}+O_{2}\rightarrow 2H_{2}O$

This means when 2 moles of hydrogen reacts with 1 mole of oxygen, 2 moles of water is produced.

Hence the ratio in which hydrogen and oxygen gas reacts is 2:1

Now if 2 mole hydrogen require 1 mole of oxygen ,then 4 mole hydrogen need 2 mole of oxygen.

$H_{2}:O_{2}=2:1$

$H_{2}:O_{2}=4:2$

Here 5 mole of oxygen is reacting but only 2 mole is required .

Oxygen is in excess.

5 0

3 years ago

Suppose 50.0g of silver nitrate is reacted with 50g of hydrochloric acid producing silver chloride and a mixture of other produc

docker41 [41]

Answer:

53.6 grams of silver chloride was produced.

Explanation:

$AgNO_3+HCl+\rightarrow AgCl+HNO_3$

Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.

This also means that total mass on the reactant side must be equal to the total mass on the product side.

Mass of silver nitrate = 50.0 g

Mass of hydrogen chloride = 50.0 g

Mass of silver chloride = x

Mass of nitric acid = 46.4 g

Mass of silver nitrate + Mass of hydrogen chloride =

Mass of silver chloride + Mass of nitric acid

[te]50.0 g+50.0 g=x+46.4 g[/tex]

$x=50.0 g+50.0 g - 46.4 g = 53.6 g$

53.6 grams of silver chloride was produced.

8 0

3 years ago

Whenever ___ energy is needed

vfiekz [6]

Well...........thanks for posting anyway.

5 0

3 years ago