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pashok25 [27]
3 years ago
10

On Earth, the three most common states of matter are Solid, Liquid, and Gas.

Chemistry
2 answers:
julsineya [31]3 years ago
3 0
TRUE you are correct but the earth is also made up of papyrus, an element.
storchak [24]3 years ago
3 0
The three main common states of matter are solid, liquid, and gas is true
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What happened when bromine reacted with aluminum?
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Answer:

The reaction begins and builds up heat. This heat causes the aluminum to melt and float on top of the liquid bromine. Wherever the two elements meet, sparks, heat, and light are given off.

Explanation:

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Noble gases have a full outer energy level and are inactive. These atoms are considered _____. neutral inert an anion a cation
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I believe that the answer  .is ( b ) inert 
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In a chemical reaction, energy can be A. released. B. absorbed. C. released or absorbed. D. neither released nor absorbed.
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C. released or absorbed.

When the energy is released the reaction is called exotermic reaction
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Niven wants to calculate the mass of MgO that is produced by the burning of 28.0 g of Mg. What is the first step in Niven’s calc
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A voltaic cell made of a Cr electrode in a solution of 1.0 M in Cr3+ and a gold electrode in a solution that is 1.0 M in Au3+.
Vikki [24]

Answer: a) Anode: Cr\rightarrow Cr^{3+}+3e^-

Cathode: Au{3+}+3e^-\rightarrow Au

b) Anode : Cr

Cathode : Au

c) Au^{3+}+Cr\rightarrow Au+Cr^{3+}

d) E_{cell}=2.14V

Explanation: - 

a) The element Cr with negative reduction potential will lose electrons undergo oxidation and thus act as anode.The element Au with positive reduction potential will gain electrons undergo reduction and thus acts as cathode.

At cathode: Au{3+}+3e^-\rightarrow Au

At anode: Cr\rightarrow Cr^{3+}+3e^-

b) At cathode which is a positive terminal, reduction occurs which is gain of electrons.

At anode which is a negative terminal, oxidation occurs which is loss of electrons.

Gold acts as cathode ad Chromium acts as anode.

c) Overall balanced equation:

At cathode: Au{3+}+3e^-\rightarrow Au     (1)

At anode: Cr\rightarrow Cr^{3+}+3e^-        (2)

Adding (1) and (2)

Au^{3+}+Cr\rightarrow Au+Cr^{3+}

d)E^0_(Cr^{3+}/Cr)= -0.74 V

E^0_(Au^{3+}/Au)= 1.40 V  

E^0{cell}=E^0{cathode}-E^0{anode}=1.40-(-0.74)=2.14V

Using Nernst equation :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Au^{3+}]}{[Cr^{3+}]^}

where,

n = number of electrons in oxidation-reduction reaction = 3

E^o_{cell} = standard electrode potential = 2.14 V

E_{cell}=2.14-\frac{0.0592}{3}\log \frac{[1.0}{[1.0]}

E_{cell}=2.14

Thus the standard potential for an electrochemical cell with the cell reaction is 2.14 V.

6 0
3 years ago
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