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Irina-Kira [14]
2 years ago
12

How many moles are there in 15.0 grams of SiO2

Chemistry
2 answers:
earnstyle [38]2 years ago
8 0

Answer:

0.25 M

Explanation:

There is 60.0843 G of SiO2 per M making 15 g equal roughly 0.25

Vinvika [58]2 years ago
7 0

n(mole)=mass: MM(molar mass)

n = 15 : 60

n = 0.25

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In the future, clean energy sources, such as solar power, may be used to create hydrogen fuel
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3 years ago
What mass of zinc is needed to react with 23.1 g of phrosphoric acid according tot he equation?
Hitman42 [59]

<u>Complete Question:</u>

what mass of zinc is needed to react with 23.1 g of phosphoric acid according tot he equation?

3 Zn + 2 H₃PO₄ = 3 H₂ + Zn₃(PO₄)₂

<u>Answer:</u>

22.98 g, the mass of zinc (Zn) is needed to react with 23.1 g of phosphoric acid according to the given equation.

<u>Explanation:</u>

Given chemical reaction:

           3 Zn + 2 H₃PO₄ = 3 H₂ + Zn₃(PO₄)₂

If the substance’ molecular weight is the number of grams required per mole, the number of moles expressed as a given quantity of substances shall correspond to the grams of that substance divided by the molecular weight. Hence,

              \text {number of moles}=\frac{\text {mass}}{\text {molar weight}}

To find no. of moles of phosphoric acid:

Given:

mass of phosphoric acid = 23.1 g

molar weight of of phosphoric acid = 97.994 = 98 g/mole

Therefore,

no. of moles of phosphoric acid =\frac{23.1}{98}=0.2357 \text { moles }

Look into the given chemical reaction and divide as the following:

If 2 moles of H₃PO₄ reacts with 3 moles of Zn then 0.2357 moles of H₃PO₄ reacts with X moles of Zn. Then,

   \text { X moles of } \mathrm{Zn}=\frac{(0.2357 \times 3)}{2}=\frac{0.707}{2}=0.3535 \text { moles of } \mathrm{Zn}

Now, calculate mass of zinc as follows, we know

molar mass of zinc is 65 g/mol

 mass\ of\ zinc = number\ of\ moles \times molar\ weight =0.3535 \times 65

Mass of zinc = 22.98 g

7 0
3 years ago
0.329 M copper (II) nitrate was reacted with 0.528 M potassium carbonate as follows: Cu (NO subscript 3 )subscript 2 italic (a q
EastWind [94]

Answer:

73.33% is the percent yield

Explanation:

Percent yield is defined as:

Actual yield (4.883g) / Theoretical yield * 100

Based on the reaction:

Cu(NO₃)₂(aq) + K₂CO₃(aq) → CuCO₃(s) + 2KNO₃(aq)

<em>1 mole of copper nitrate reacts per mol of potassium carbonate.</em>

<em />

To solve this question we must find limiting reactant. With limiting reactant we can find the theoretical moles of solid produced and its mass as follows:

<em>Moles Cu(NO₃)₂:</em>

0.1639L * (0.329mol / L) = 0.0539 moles

<em>Moles K₂CO₃:</em>

0.1639L * (0.528mol / L) = 0.0865 moles

As the reaction is 1:1, the limiting reactant is Cu(NO₃)₂.

1 mol of Cu(NO₃)₂ produces 1 mol of CuCO₃. That means theoretical moles produced are 0.0539 moles. And the mass is:

<em>Mass CuCO₃ -Molar mass: 123.55g/mol-</em>

0.0539 moles * (123.55g / mol) = 6.659g of CuCO₃ is the theoretical mass

And percent yield:

4.883g / 6.659g * 100

<h3>73.33% is the percent yield</h3>
3 0
3 years ago
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