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enyata [817]
3 years ago
10

___Fe + ___O2 ___Fe2O3

Chemistry
1 answer:
Dafna11 [192]3 years ago
4 0

Answer:

4 Fe + 3 O2 -> 2Fe2O3

Explanation:

For the equation to be balanced with whole numbers, you need to double the amount of Fe2O3. This gives 6 oxygen molecules and 4 Fe molecules.

So the number of atoms will be Fe = 4 and O = 6.

For the visual Model Key, you will most likely have, 4 separate Fe molecules and 3 oxygen molecules (since oxygen exists as a diatomic - 2 oxygen molecules are attached to each other). For Fe2O3 you will have 2 molecules that go O-Fe-O-Fe-O.

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How many phosphorus atoms are represented in the formula?
Virty [35]

Answer:

i believe 4

Explanation:

hope this helps :)

7 0
3 years ago
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7. How many moles are there in 4.6 gms of Sodium(Na)?
Marizza181 [45]

Answer:

0.2mol

Explanation:

mol = mass/mr

mass = 4.6g

mr = 23

mol = 4.6/23

= 0.2mol

7 0
3 years ago
4 Al + 3O2 → 2Al2O3 If 14.6 grams Al are reacted, how many liters of O2 at STP would be required?
melomori [17]

Answer: 9.08 L

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}\times{\text{Molar Mass}}    

\text{Moles of} Al=\frac{14.6g}{27g/mol}=0.54moles

4Al+3O_2\rightarrow 2Al_2O_3

According to stoichiometry :

4 moles of Al require  = 3 moles of O_2

Thus 0.54 moles of Al will require=\frac{3}{4}\times 0.54=0.405moles  of O_2

Standard condition of temperature (STP)  is 273 K and atmospheric pressure is 1 atm respectively.

According to the ideal gas equation:

PV=nRT

P = Pressure of the gas = 1 atm

V= Volume of the gas = ?

T= Temperature of the gas = 273 K      

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas= 0.405

V=\frac{nRT}{P}=\frac{0.405\times 0.0821\times 273}{1}=9.08L

Thus 9.08 L of O_2 at STP would be required

6 0
3 years ago
Krypton is named after the Greek word that means “secret.” Which explains why krypton was most likely given this name?
GaryK [48]

Answer:

C) Krypton is a noble gas, so it was difficult for chemists to find it, as though it was a secret.

Explanation:

4 0
3 years ago
Read 2 more answers
How many kilograms of a fertilizer are made of pure P2O5 would be required to supply 1.69 kilogram of phosphorus to the soil?
Alekssandra [29.7K]

Answer:

3.89 kg P2O5 must be used to supply 1.69 kg Phosphorus to the soil.

Explanation:

The molecular mass of P2O5 is

P2 = 2* 31 =           62

O5 = 5 *<u> 16 =         80</u>

Molecular Mass = 142

Set up a Proportion

142 grams P2O5 supplies 62 grams of phosphorus

x    kg P2O5        supplies 1.69 kg of phosphorus

Though this might be a bit anti intuitive, you don't have to convert the units for this question. The ratio is all that is important.

142/x = 62/1.69            Cross multiply

142 * 1.69 = 62x           combine the left

239.98 = 62x               Divide by 62

239.98/62 = x

3.89 kg of P2O5 must be used.

3 0
3 years ago
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