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Pie
3 years ago
10

How many total atoms are in 0.920 g of P2O5?

Chemistry
2 answers:
lions [1.4K]3 years ago
8 0
Molar mass P2O5 = 31 x 2 + 16 x 5 => 142 g/mol


142 g ---------------- 6.02 x 10²³ molecules
0.920g g ------------ ( molecules )

molecules = 0.920 x ( 6.02 x 10²³ ) / 142

molecules = 5.53 x 10²³ / 142

= 3.89 x 10²¹ molecules

1 molecule P2O5 -------------------------- 7 atoms
3.89 x 10²¹ molecules -------------------- ( atoms )

atoms = ( 3.89 x 10²¹) x 7 / 1

atoms = 2.72 x 10²² atoms of P2O5

hope this helps!
SSSSS [86.1K]3 years ago
5 0
Given the mass of a compound, the total number of atoms can be determined by converting first the mass to moles and then multiplying the moles to Avogadro's number (6.022 x 10^23 atoms/mole). In this case, the answer is 3.9 x10^21 atoms
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What force works against gravity as water infiltrates the soil and moves
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Answer is option B . This is because water is said to be highly permeable to the underground soil and thus nourishes it , whereas capillary action will make the water flow upward sllowly , but the water is going underground so it is permeability. Also soil is porous too , but that's only if the water is in the soil , here the water is caused to go underground by some force , so porosity isnt the right option

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Which property best indicates that a compound contains an ionic bond?
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They dissociate into positive and negative ions in the solution.

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Zinc metal and aqueous silver nitrate react to give Zn(NO3)2(aq) plus silver metal. When 5.00 g of Zn(s) and solution containing
Fittoniya [83]

Answer : The percent yield is, 83.51 %

Solution : Given,

Mass of Zn = 5.00 g

Mass of AgNO_3 = 25.00 g

Molar mass of Zn = 65.38 g/mole

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Molar mass of Ag = 107.87 g/mole

First we have to calculate the moles of Zn and AgNO_3.

\text{ Moles of }Zn=\frac{\text{ Mass of }Zn}{\text{ Molar mass of }Zn}=\frac{5.00g}{65.38g/mole}=0.0765moles

\text{ Moles of }AgNO_3=\frac{\text{ Mass of }AgNO_3}{\text{ Molar mass of }AgNO_3}=\frac{25.00g}{168.97g/mole}=0.1479moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

Zn+2AgNO_3\rightarrow Zn(NO_3)_2+2Ag

From the balanced reaction we conclude that

As, 2 mole of AgNO_3 react with 1 mole of Zn

So, 0.1479 moles of AgNO_3 react with \frac{0.1479}{2}=0.07395 moles of Zn

From this we conclude that, Zn is an excess reagent because the given moles are greater than the required moles and AgNO_3 is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of Ag

From the reaction, we conclude that

As, 2 mole of AgNO_3 react to give 2 mole of Ag

So, 0.1479 moles of AgNO_3 react to give 0.1479 moles of Ag

Now we have to calculate the mass of Ag

\text{ Mass of }Ag=\text{ Moles of }Ag\times \text{ Molar mass of }Ag

\text{ Mass of }Ag=(0.1479moles)\times (107.87g/mole)=15.95g

Theoretical yield of Ag = 15.95 g

Experimental yield of Ag = 13.32 g

Now we have to calculate the percent yield.

\% \text{ yield}=\frac{\text{ Experimental yield of }Ag}{\text{ Theretical yield of }Ag}\times 100

\% \text{ yield}=\frac{13.32g}{15.95g}\times 100=83.51\%

Therefore, the percent yield is, 83.51 %

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