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Serjik [45]
2 years ago
7

Having a difficult time please help me ;( I would appreciate whoever helps me thank you! If you can explain that would be awesom

e thank you!

Chemistry
1 answer:
SOVA2 [1]2 years ago
3 0

Answer: A. 11

Explanation: The balance equation is:

C7H16 + 11 O2 => 7CO2 + 8H2O

This is a combustion reaction where a hydrocarbon reacts with oxygen gas to form CO2 and H2O.

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For some hypothetical metal, the equilibrium number of vacancies at 600°C is 1 × 1025 m-3. If the density and atomic weight of t
makvit [3.9K]

Answer:

\frac{N_{v}}{N}=1.92*10^{-4}

Explanation:

First of all we need to find the amount of atoms per volume (m³). We can do this using the density and the molar mass.

7.40 \frac{g}{cm^{3}}*\frac{1mol}{85.5 g}*\frac{6.023*10^{23}atoms}{1mol}*\frac{1000000 cm^{3}}{1m^{3}}=5.21*10^{28}\frac{atoms}{m^{3}}

Now, the fraction of vacancies is equal to the N(v)/N ratio.

  • N(v) is the number of vacancies 1*10^{25}m^{-3}
  • N is the number of atoms per volume calculated above.

Therefore:  

The fraction of vacancies at 600 °C will be:

\frac{N_{v}}{N}=\frac{1*10^{25}}{5.21*10^{28}}  

\frac{N_{v}}{N}=1.92*10^{-4}

I hope it helps you!

 

7 0
3 years ago
What is the mole fraction of ethanol in a mixture of 0.25 mol of ethanol and 0.4 mol of methanol? Report your answer to the hund
snow_tiger [21]

Answer:

0.3846

Explanation:

i used fractions

6 0
3 years ago
What is water condensing on a cold glass an example of? and explain
Nana76 [90]
The answer is
b)state of matter 

because water is changing from a gas to liquid
4 0
3 years ago
If 3.0 moles of x and 4.0 moles of y react according to the hypothetical reaction below, how many moles of the excess reactant w
Umnica [9.8K]
Answer is: <span>1.0 mol X left over. 
</span>Chemical reaction: X + 2Y → XY₂.
n(X) = 3,0 mol, excess reactant.
n(Y) = 4,0 mol, limiting reagent.
n - amount of substance.
from reaction: n(X) : n(Y) = 1 : 2.
n(X) : 4 mol = 1 : 2.
n(X) = 2 mol, that reacts.
excess of X: 3 mol - 2 mol = 1 mol.

4 0
3 years ago
If 5.40 kcal of heat is added to 1.00 kg of water at 100⁰C, how much steam at 100⁰C is produced? Show all calculations leading t
Eddi Din [679]
Heat of vaporization of water = 540 cal/g
m=1000 g
energy supplied = 5.4 kcal=5400 cal
T1=T2=100 deg. C
so all energy is used to convert to steam
mass of steam produced = 5400 cal /(540 cal/g)
=5400/540 cal *g/cal
=10 g
8 0
3 years ago
Read 2 more answers
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