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Mazyrski [523]
3 years ago
5

4.5 X 6.02214076 x 10^23

Chemistry
1 answer:
Rufina [12.5K]3 years ago
5 0

Answer:

I really don't know but I guess

Explanation:

2.7 would be the answer or 2.70

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If air is heated to 100F above normal room air temperature, what happens to the air?
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The molecules will start to move faster and rise while pushing the slower molecules down until they are heated and when the pressure finally builds up and is released

7 0
4 years ago
04.05 mol
victus00 [196]

Answer:

34.8 g

Explanation:

Answer:

We have the masses of two reactants, so this is a limiting reactant problem.

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.  

Mᵣ:         123.90    70.91      208.24

                 P₄   +   20Cl₂ ⟶ 4PCl₅

Mass/g:   46.0       32.0

2. Calculate the moles of each reactant  

\text{moles of P}_{4} = \text{46.0 g P}_{4} \times \dfrac{\text{1 mol P}_{4}}{\text{123.90 g P}_{4}} = \text{0.3713 mol P}_{4}\\\\\text{moles of Cl}_{2} = \text{32.0 g Cl }_{2} \times \dfrac{\text{1 mol Cl }_{2}}{\text{70.91 g Cl }_{2}} = \text{0.4513 mol Cl }_{2}

3. Calculate the moles of PCl₅ we can obtain from each reactant

From P₄:

The molar ratio is 4 mol PCl₅:4 mol P₄

\text{Moles of PCl}_{5} = \text{0.3713 mol P}_{4} \times \dfrac{\text{4 mol PCl}_{5}}{\text{4 mol P}_{4}} = \text{0.3713 mol PCl}_{5}

From Cl₂:

The molar ratio is 4 mol PCl₅:20 mol Cl₂

\text{Moles of PCl}_{5} =  \text{0.4513 mol Cl}_{2}\times \dfrac{\text{4 mol PCl}_{5}}{\text{20 mol Cl}_{2}} = \text{0.090 26 mol PCl}_{5}

4. Identify the limiting and excess reactants

The limiting reactant is chlorine, because it gives the smaller amount of PCl₅.

The excess reactant is phosphorus.

5. Mass of excess reactant

(a) Moles of P₄ reacted

The molar ratio is 1 mol P₄:20 mol Cl₂

\text{Moles reacted} = \text{0.4513 mol Cl}_{2} \times \dfrac{\text{4 mol P}_{4}}{\text{20 mol Cl}_{2}} = \text{0.090 26 mol P}_{4}

(b) Mass of P₄ reacted

\text{Mass reacted} = \text{0.090 26 mol P}_{4} \times \dfrac{\text{123.90 g P}_{4}}{\text{1 mol P}_{4}} = \text{11.18 g P}_{4}

(c) Mass of P₄ remaining

Mass remaining = original mass – mass reacted = (46.0 - 11.18) g = 34.8 g P₄

4 0
4 years ago
When 120 g of carbon reacts completely with 320 g of oxygen the mass of carbon dioxide formed will be?
olga2289 [7]
440 cause mass cant be created or destroyed
6 0
3 years ago
Some properties of matter depend on how much matter there is. Put an X next to all of the statements you think are true about pr
ella [17]

Answer:

Its B and D :)

Explanation:

I saw the answer key.

3 0
3 years ago
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