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3 years ago

PLEASE HELP ME ON THIS

Chemistry

1 answer:

lisabon 2012 [21]3 years ago

3 0

Answer:

The conductance will increase as the concentration of the electrolyte is increased.

Explanation:

The ions are what carry the charges from one electrode to another. The more there are, the easier it is for electrons to get across the solution of electrolyte,

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What must be true for a spontaneous reaction in an electrochemical cell? The overall cell potential must be positive. The overal

yanalaym [24]

Answer:

The overall cell potential must be positive.

Explanation:

What must be true for a spontaneous reaction in an electrochemical cell?

The overall cell potential must be positive. YES. This is by convention.

The overall cell potential must be negative. NO. By convention, a negative cell potential means the cell is not spontaneous.

The cathode’s standard reduction potential must be positive. NO. It only has to be higher than the anode's standard reduction potential.

The cathode’s standard reduction potential must be negative. NO. It only has to be higher than the anode's standard reduction potential.

7 0

3 years ago

Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing element?

Marina CMI [18]

Answer:

Dmitri Mendeleev

Explanation:

Dmitri Mendeleev a Russian Chemist arranged elements on the periodic table according to their atomic mass. He used this arrangement to predict some of the properties of the missing element.

Dmitri Mendeleev around 1869 described the periodic table.
The table was based on the periodic law which states that "chemical properties of elements are a periodic function of their atomic weights".
In the Mendeleev table, elements are arranged by atomic weights with recurring properties in a periodic manner.

3 0

3 years ago

A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3. Determine the equilibrium pressure of NO2 if Kp for the reac

dlinn [17]

Explanation:

Reaction equation for this reaction is as follows.

$NO(g) + SO_{3}(g) \rightarrow NO_{2}(g) + SO_{2}(g)$

It is given that $K_{p}$ = 0.0118.

According to the ICE table,

$NO(g) + SO_{3}(g) \rightarrow NO_{2}(g) + SO_{2}(g)$

Initial: 0.86 0.86 0 0

Change: -x -x +x +x

Equilibrium: 0.86 - x 0.86 - x x x

Hence, value of $K_{p}$ will be calculated as follows.

$K_{p} = \frac{P_{NO_{2}} \times P_{SO_{3}}}{P_{NO} \times P_{SO_{3}}}$

0.0118 = $\frac{x \times x}{(0.86 - x)^{2}}$

x = 0.084 atm

Thus, we can conclude that $P_{NO_{2}}$ is 0.084 atm.

4 0

4 years ago

Where does cellular respiration occur?

lukranit [14]

The answer to the question is c! If u need me to explain I will in the comments but I hope this helped ;)

4 0

3 years ago

In thermodynamics, we determine the spontaneity of a reaction by the sign of ΔG. In electrochemistry, spontaneity is determined

faltersainse [42]

Answer:

For A: The standard cell potential of the reaction is 4.4 V

For B: The standard Gibbs free energy of the reaction is $-8.50\times 10^5J$

For C: The reaction is spontaneous as written.

Explanation:

For A:

The given chemical reaction follows:

$2Li(s)+Cl_2(g)\rightarrow 2Li^+(aq.)+2Cl^-(aq.)$

The given half reaction follows:

Oxidation half reaction: $Li(s)\rightarrow Li^+(aq.)+e^-;E^o_{Li^+/Li}=-3.04V$ ( × 2)

Reduction half reaction: $Cl_2(g)+2e^-\rightarrow 2Cl^-(aq.);E^o_{Cl_2/2Cl^-}=+1.36V$

The substance having highest positive $E^o$ potential will always get reduced and will undergo reduction reaction.

Here, chlorine will undergo reduction reaction will get reduced.

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

$E^o_{cell}=1.36-(-3.04)=4.4V$

Hence, the standard cell potential of the reaction is 4.4 V

For B:

Relationship between standard Gibbs free energy and standard electrode potential follows:

$\Delta G^o=-nFE^o_{cell}$

where,

n = number of electrons transferred = $2mol\text{ e}^-$

F = Faradays constant = $96500J/V.mol\text{ e}^-$

$E^o_{cell}$ = standard cell potential = 4.4 V

Putting values in above equation, we get:

$\Delta G^o=-2\times 96500\times 4.4=-849200J=-8.50\times 10^5J$

Hence, the standard Gibbs free energy of the reaction is $-8.50\times 10^5J$

For C:

For a reaction to be spontaneous, the standard Gibbs free energy change of the reaction must be negative.

From above, the standard Gibbs free energy change of the reaction is coming out to be negative.

Hence, the reaction is spontaneous as written.

7 0

4 years ago

PLEASE HELP ME ON THIS ​

PLEASE HELP ME ON THIS