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Marrrta [24]
3 years ago
11

Which shows the correct relationship?

Chemistry
2 answers:
erastova [34]3 years ago
7 0

Answer: B.) E^0_{cell} > 0 = spontaneous reaction

Explanation:

The standard emf of a cell is related to Gibbs free energy by following relation:

\Delta G=-nFE^0

\Delta G = gibbs free energy

n= no of electrons gained or lost

F= faraday's constant

E^0 = standard emf

when \Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

Thus reaction is spontaneous when E^0= +ve

Thus reaction is non spontaneous when E^0= -ve

Thus reaction is in equilibrium when E^0= 0.

Andrews [41]3 years ago
4 0
I think the correct answer from the choices listed above is option B. The correct relationship would be Eo cell > 0 = spontaneous reaction. For a spontaneous reaction, Ecell<span> is </span>positive<span> and ΔG (Gibbs free energy, used to determine if a reaction occurs spontaneously) is </span>negative<span>. Hope this answers the question.</span>
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At what speed does all electromagnetic radiation travel?
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10 to the power of 8

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4 0
2 years ago
What is the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen
natta225 [31]
Carbon(C):
number of moles= mass/molar mass(Mr)
=65.5/12
=5.5 moles

Hydrogen(H):
number of moles=mass/molar mass (Mr)
=5.5/1
=5.5 moles

Oxygen (O):
number of moles = mass/molar mass (Mr)
=29.0/16
=1.8 moles

EF= lowest number of moles over each of the elements

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6 0
2 years ago
what is the limiting reactant when 1.50g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advan
PSYCHO15rus [73]
<h3>Answer:</h3>

Limiting reactant is Lithium

<h3>Explanation:</h3>

<u>We are given;</u>

  1. Mass of Lithium as 1.50 g
  2. Mass of nitrogen is 1.50 g

We are required to determine the rate limiting reagent.

  • First, we write the balanced equation for the reaction

6Li(s) + N₂(g) → 2Li₃N

From the equation, 6 moles of Lithium reacts with 1 mole of nitrogen.

  • Second, we determine moles of Lithium and nitrogen given.

Moles = Mass ÷ Molar mass

Moles of Lithium

Molar mass of Li = 6.941 g/mol

Moles of Li = 1.50 g ÷ 6.941 g/mol

                   = 0.216 moles

Moles of nitrogen gas

Molar mass of Nitrogen gas is 28.0 g/mol

Moles of nitrogen gas = 1.50 g ÷ 28.0 g/mol

                                     = 0.054 moles

  • According to the equation, 6 moles of Lithium reacts with 1 mole of nitrogen.
  • Therefore, 0.216 moles of lithium will require 0.036 moles (0.216 moles ÷6) of nitrogen gas.
  • On the other hand, 0.054 moles of nitrogen, would require 0.324 moles of Lithium.

Thus, Lithium is the limiting reagent while nitrogen is in excess.

7 0
3 years ago
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