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MAVERICK [17]
3 years ago
9

The total number of atoms represented by the formula Fe3(PO4)2 is

Chemistry
2 answers:
In-s [12.5K]3 years ago
8 0
C is the answer 3 + 2 +8 = 13
horsena [70]3 years ago
7 0

Answer:

C.

Explanation:

We have to keep in mind for this question that we have to take into account the <u>subscripts</u>.

Fe_3(PO_4)_2

The <u>subscript will affect only the number in the left</u>, so the first part would be:

Fe_3

In this part we will have 3 iron atoms. Then we will have:

(PO_4)_2

In the PO_4 we will have 1 atom of P and 4 atoms of O. (When we dont have any number as subscript we have to <u>assume that we have a "1</u>")

Then we have a "2" out side the the parenthesis (PO_4)_2, so we have to multiply by "2" all the <u>atoms inside the parenthesis</u>, so:

1 atom of P x 2 = 2

4 atoms of O x 2 = 8

So, in total we will have:

3 atoms of Fe + 8 atoms of O + 2 atoms of P = <u>13 atoms</u>

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Luba_88 [7]
Dry air is a mixture of nitrogen, oxygen, carbon dioxide etc.
air is a mixture of gases 78% nitrogen an 21% oxygen and other components.
7 0
3 years ago
The vapor pressure of water at 25.0°c is 23.8 torr. determine the mass of glucose (molar mass = 180 g/mol) needed to add to 500.
svp [43]
Q: A
according to this formula, we can get the mole fraction of water (n):
P(solu) = n Pv(water)
when we have Pv(solu) = 22.8 and Pv(water) = 23.8 so by substitution:
22.8 = n * 23.8
n= 0.958
- we need to get the moles of glucose:
moles of water = 500 g(mass weight) / 18 (molar weight)= 27.7 mol
n = moles of water / ( moles of water + moles of glucose)
0.958   = 27.7 / ( 27.7+ moles of glucose)
0.958 moles of glucose + 26.5 = 27.7
0.968 moles of glucose = 1.2
moles of glucose = 1.253 mol
∴ the mass of glucose = no.of glucose moles x molar mass 
                                      = 1.253 x 180 = 225.5 g
Q: B
here we also need to get n (mole fraction of water )by using this formula:
Pv(solu) = n Pv(water)
when we have Pv(solu)=132 & Pv(water)=150 so, by substition:
132= n * 150
n = 0.88
so, mole fraction of solution = 1 - 0.88 = 0.12
and we can get after that the moles of water = (mass weight / molar mass)
- no.moles of water = 85 g / 18 g/mol = 4.7 moles
- total moles in solution = moles of water / moles fraction of water 
                                        = 4.7 / 0.88 = 5.34 moles 
∴ moles of the solution = total moles in solu - moles of water 
                                       = 5.34 - 4.7 = 0.64 moles solute
∴ the molar mass of the solute = mass weight of solute / no.of moles of solute
                                                    = 53.8 / 0.64 = 84 g/mole

Q: C

moles of urea (NH2)2 CO = mass weight / molar mass
                                           = 4.49 g / 60 g /mol
                                           = 0.07 mol
moles of methanol = mass weight / molar mass 
                                 = 39.9  g / 32  g/mol = 1.25 mol
moles fraction of methanol = moles of methanol / (moles of methanol + moles of urea )
moles fraction of methanol = 1.25 / ( 1.25+0.07) = 0.95
by substitution in Pv formula we will be able to get the vapour pressure of the solu :
Pv(solu) = n P°v
Pv(solu) = 0.95 * 89 mm Hg 
∴Pv(solu) = 84.55 mmHg


 
7 0
3 years ago
100 POINTS HELP WILL GIVE BRAINLIEST
vodomira [7]

b. testing the hypothesis

6 0
1 year ago
Which equation demonstrates that nuclear fusion forms elements that are heavier than helium
GrogVix [38]

Answer: The correct option is 2.

Explanation: There are two types of nuclear reactions:

1) Nuclear fission: These reactions are defined as the reactions in which a heavier unstable nuclei breaks into two or more smaller stable nuclei.

2) Nuclear fusion: These reactions are the ones where two smaller nuclei fuse together or combine together to form a larger nuclei.

In the question, we need to find the fusion reaction which forms elements heavier than helium.

Option 1: In this fusion reaction occurs but the nuclei is Helium itself.

Option 2: In this also fusion reaction occurs and the nuclei is heavier than Helium which is Neon.

_8^{16}\textrm{O}+_2^4\textrm{He}\rightarrow _{10}^{20}\textrm{Ne}

Option 3 and Option 4: These two reactions are nuclear fission reactions of Uranium-235 because one heavier element is breaking into more than 2 products.

Hence, the correct option is 2.

8 0
3 years ago
Read 2 more answers
A 0.1 gram sample of an unknown liquid is vaporized completely at 70 degrees C to fill a 750mL flask. The pressure is 0.05951atm
Deffense [45]

Answer:

The molar mass of the liquid 62.89 g/mol

Explanation:

Step 1: Data given

Mass of the sample = 0.1 grams

Temperature = 70°C

Volume = 750 mL

Pressure = 0.05951 atm

Step 2: Calculate the number of moles

p*V = n*R*T

n = (p*V)/(R*T)

⇒ with n = the number of moles gas = TO BE DETERMINED

⇒ with p = The pressure = 0.05951 atm

⇒ with V = The volume of the flask = 750 mL = 0.750 L

⇒ with R = The gasconstant = 0.08206 L*atm/K*mol

⇒with T = the temperature = 70 °C = 343 Kelvin

n = (0.05951 *0.750)/(0.08206*343)

n = 0.00159 moles

Step 3: Calculate molar mass

Molar mass = mass / moles

Molar mass =0.1 gram /  0.00159 moles

Molar mass = 62.89 g/mol

The molar mass of the liquid 62.89 g/mol

6 0
3 years ago
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