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1 year ago

In a voltaic (galvanic) cell, oxidation occurs at the _ and is where _ in the salt bridge moves toward.

1 answer:

4 0

In a voltaic (galvanic) cell, oxidation occurs at the <u>anode</u> and is where <u>anions</u> in the salt bridge moves toward.

<h3>What is Galvanic Cell ?</h3>

Galvanic Cell or Voltaic Cell is an electrochemical cell that converts the energy of spontaneous redox reactions into electrical energy. In galvanic cell oxidation occurs at the anode and reduction occurs at the cathode. The anode is positive and cathode is negative, anode attracts anions from solution in an electrolytic cell.

Thus from the above conclusion we can say that In a voltaic (galvanic) cell, oxidation occurs at the <u>anode</u> and is where <u>anions</u> in the salt bridge moves toward.

Learn more about the Galvanic Cell here: brainly.com/question/15096829

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An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction At

anygoal [31]

Answer: [N2]₀ = 10M and [H2]₀ = 11M

Explanation: To calculate the initial concentration, you would have to set up an ICE table, which is an organized way of tracking known quantities or the ones you want to find. ICE stands for:

I is initial amount;

C is change in concentration;

E is for equilibrium concentration;

For the mixture,

N2 3H2 2NH3

I [N2]₀ [H2]₀ 0

C - x -3x +2x

E [N2]₀ - x =8 [H2]₀ - 3x =5 2x =4

With the product, we can find "x":

2x=4

x=2M

With x=2, find the concentrations:

[N2]₀ - x = 8

[N2]₀ = 10M

[H2]₀ - 3x = 5

[H2]₀ = 11M

The initial concentrations of nitrogen gas [N2] is 10.0 M and of hydrogen gas [H2] is 11.0 M.

8 0

3 years ago

Read 2 more answers

1. What would happen to the position of equilibrium when the following changes are made to the reaction below? 2Hg3O (g) ↔ 6Hg (

Mademuasel [1]

What is your answer I can help you)

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3 years ago

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The dissociation of sulfurous acid (H2SO3) in aqueous solution occurs as follows:

aksik [14]

Answer:

The [SO₃²⁻]

Explanation:

From the first dissociation of sulfurous acid we have:

H₂SO₃(aq) ⇄ H⁺(aq) + HSO₃⁻(aq)

At equilibrium: 0.50M - x x x

The equilibrium constant (Ka₁) is:

$K_{a1} = \frac{[H^{+}] [HSO_{3}^{-}]}{[H_{2}SO_{3}]} = \frac{x\cdot x}{0.5 - x} = \frac {x^{2}}{0.5 -x}$

With Ka₁= 1.5x10⁻² and solving the quadratic equation, we get the following HSO₃⁻ and H⁺ concentrations:

$[HSO_{3}^{-}] = [H^{+}] = 7.94 \cdot 10^{-2}M$

Similarly, from the second dissociation of sulfurous acid we have:

HSO₃⁻(aq) ⇄ H⁺(aq) + SO₃²⁻(aq)

At equilibrium: 7.94x10⁻²M - x x x

The equilibrium constant (Ka₂) is:

$K_{a2} = \frac{[H^{+}] [SO_{3}^{2-}]}{[HSO_{3}^{-}]} = \frac{x^{2}}{7.94 \cdot 10^{-2} - x}$

Using Ka₂= 6.3x10⁻⁸ and solving the quadratic equation, we get the following SO₃⁻ and H⁺ concentrations:

$[SO_{3}^{2-}] = [H^{+}] = 7.07 \cdot 10^{-5}M$

Therefore, the final concentrations are:

[H₂SO₃] = 0.5M - 7.94x10⁻²M = 0.42M

[HSO₃⁻] = 7.94x10⁻²M - 7.07x10⁻⁵M = 7.93x10⁻²M

[SO₃²⁻] = 7.07x10⁻⁵M

[H⁺] = 7.94x10⁻²M + 7.07x10⁻⁵M = 7.95x10⁻²M

So, the lowest concentration at equilibrium is [SO₃²⁻] = 7.07x10⁻⁵M.

I hope it helps you!

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3 years ago

Increasing technology addiction among the youth write a letter to editor

ruslelena [56]

Answer:

these two would help you

Explanation:

have a good day ᕕ( ᐛ )ᕗ

6 0

2 years ago

How many moles in 843.211 grams of c6h12o6?

leonid [27]

Molar mass C6H12O6 = 12 x 6 + 1 x 12 + 16 x 6 = 180 g/mol

1 mole ------------ 180 g
( moles ) --------- 843.211 g

moles = 843.211 x 1 / 180

moles = 843.211 / 180

= 4,684 moles of C6H12O6

3 0

3 years ago

In a voltaic (galvanic) cell, oxidation occurs at the _____ and is where _____ in the salt bridge moves toward.

In a voltaic (galvanic) cell, oxidation occurs at the _ and is where _ in the salt bridge moves toward.