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tatyana61 [14]
2 years ago
9

Help with the 3rd question plslsls I’ll brainlist.

Chemistry
1 answer:
Brilliant_brown [7]2 years ago
4 0

1 - energy 2- heat 3 -plant

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Quarks are<br> A A Fact<br> B Fiction<br> C Both of the above<br> D Neither of the above
stiks02 [169]
I’d say A. They are theoretical in the fact that they have not been observed directly, but have been confirmed to exist through experimentation.
7 0
2 years ago
How many molecules of O2 will be required to produce 28.8 g of water?
Mrac [35]
I think 1.67 x 10^20
5 0
3 years ago
The measure of the attraction that an atom has for electrons involved in chemical bonds is known as: ? electron affinity / radio
swat32
The answer is the last option. Electronegativity is the measure of the attraction that an atom has for electrons involved in chemical bonds.  It relates to covalent bonds where electrons are shared. The Pauling scale is the most used.
5 0
3 years ago
Read 2 more answers
Describe the relationship between the radius of a cation and that of the atom from which it is formed. a. cations are much small
koban [17]
<h3><u>Answer;</u></h3>

Cations are much smaller than their corresponding parent

<h3><u>Explanation;</u></h3>
  • Parent atom has more electrons and thus the effective nuclear charge on each electron is less.
  • When a cation is formed electron(s) is/are lost. Thus the effective nuclear charge or simply put, the attraction of the nucleus towards the electrons increases. Therefore, due to greater pull, the nucleus pulls the shells towards it, there by reducing the size, which makes cations smaller than their corresponding parent.
3 0
3 years ago
If the reduction reaction has a reduction potential of 0.1 V, and the oxidation reaction has a reduction potential of -0.4V, and
aleksley [76]

Answer : The value of ΔG expressed in terms of F is, -1 F

Explanation :

First we have to calculate the standard electrode potential of the cell.

E^o=E^o_{cathode}-E^o_{anode}

or,

E^o=E^o_{reduction}-E^o_{oxidation}

E^o=(0.1V)-(-0.4V)=+0.5V

Now we have to calculate the standard cell potential.

Formula used :

\Delta G^o=-nFE^o

where,

\Delta G^o = Gibbs free energy = ?

n = number of electrons = 2

F = Faraday constant

E^o = standard e.m.f of cell = +0.5 V

Now put all the given values in this formula, we get the Gibbs free energy.

\Delta G^o=-(2\times F\times 0.5)

\Delta G^o=-1F

Therefore, the value of ΔG expressed in terms of F is, -1 F

5 0
3 years ago
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