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2 years ago

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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3 years ago

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

Hitman42 [59]

Complete Question:

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

Answer:

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

Explanation:

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)

1 mole of copper nitrate reacts per mol of potassium carbonate.

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:

Moles Cu(NO₃)₂:

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

Moles K₂CO₃:

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:

Mass CuCO₃ -Molar mass: 123.55g/mol-

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>

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3 years ago