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4 years ago

Calculate LaTeX: \DeltaΔGº for a voltaic cell with Eºcell = +0.24 V if the overall reaction involves a 3 electron reduction.

Chemistry

1 answer:

umka2103 [35]4 years ago

7 0

Answer:

-69 kJ

Explanation:

Step 1: Given data

Standard cell potential (E°cell): +0.24 V

Electrons involved (n): 3 mol

Step 2: Calculate the standard Gibbs free energy change (ΔG°) for the voltaic cell

We will use the following expression.

ΔG° = -n × F × E°cell

where,

F is Faraday's constant (96,485 C/mol e⁻)

ΔG° = -n × F × E°cell

ΔG° = -3 mol e⁻ × 96,485 C/mol e⁻ × 0.24 V

ΔG° = -69 kJ

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An object of mass 10.0 kg is initially at rest. A 100 N force causes it to move horizontally through a distance of 6.00 m. What

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Answer:

The answer to the question is

The change in the kinetic energy of the object is 600 J

Explanation:

The known variables are,

Mass of object, m = 100 kg

Force of object, F = 100 N

The relation for kinetic energy = KE = $\frac{1}{2} * m * v^{2}$ = 0.5·m·v²

Therefore to find v we first find the acceleration from

F = m·a =10.0 kg × a = 100 N,

Where a = acceleration of the object =100/10 = 10 m/s²

To find the velocity, v, we use the relationship

v² = u² + 2 × a × S, where S is the distance of motion = 6.00 m and u is the initial velocity, u = 0 m/s, therefore

v² = 0 + 2 × 10 m/s² × 6 m = 120 m²/s² or v = 10.95 m/s

Therefore KE = 0.5 × 10 kg × (10.95 m/s)² = 600 J

where the initial velocity, u = 0 m/s

Initial kinetic energy of the object = KE₁ = 0.5 × 10 × 0² = 0

The change in kinetic energy of the object = 600 J - 0 J = 600 J

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4 years ago

How many molecules are in one mole of NH3?

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Answer:

1 mole of NH3 has 6.023×10^23 molecules.

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3 years ago

What tools would you use to measure the density of a rectangular block?

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A scale and a ruler. The scale to measure the mass, and a ruler to measure the volume.

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3 years ago

The daily output of stomach acid (gastric juice) is 1000 to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1

Semmy [17]

Answer:

B.) 2 HCl(aq) + CaCO₃(s) → CaCl₂(aq) + H₂O(l) + CO₂(g)

C.) 7.4 × 10² mL

D.) 2 HCl(aq) + Mg(OH)₂(aq) → MgCl₂(aq) + H₂O(l)

E.) 1.3 × 10³ mL

Explanation:

The daily output of stomach acid (gastric juice) is 1000 to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1.49.

We can calculate the concentration of H⁺ using the definition of pH.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog (-1.49) = 0.0324 M

Since HCl is a strong monoprotic acid, we can consider this to be the concentration of HCl as well.

B.) One chewable tablet of the antacid Maalox contains 600 mg of CaCO₃. Enter the neutralization equation. Express your answer as a molecular equation including phases.

The neutralization equation is:

2 HCl(aq) + CaCO₃(s) → CaCl₂(aq) + H₂O(l) + CO₂(g)

C.) Given that one chewable tablet of the antacid Maalox contains 600 mg of CaCO₃, calculate the milliliters of stomach acid neutralized by two tablets of Maalox. Express the volume in milliliters to two significant figures.

We can establish the following relations:

Each tablet has 600 mg (0.600 g) of CaCO₃.
The molar mass of CaCO₃ is 100.09 g/mol.
The molar ratio of HCl to CaCO₃ is 2:1.
The concentration of HCl is 0.0324 mol/L.

The mililiters of HCl that neutralize 2 tablets of Maalox are:

$2Tablet.\frac{0.600gCaCO_{3}}{1Tablet} .\frac{1molCaCO_{3}}{100.09gCaCO_{3}} .\frac{2molHCl}{1molCaCO_{3}} .\frac{1000mLHCl}{0.0324molHCl} =7.4 \times 10^{2} mLHCl$

D.) The antacid milk of magnesia contains 400 mg of Mg(OH)₂ per teaspoon. Enter the neutralization equation. Express your answer as a molecular equation including phases.

The neutralization equation is:

2 HCl(aq) + Mg(OH)₂(aq) → MgCl₂(aq) + H₂O(l)

E.) Given that the antacid milk of magnesia contains 400 mg of Mg(OH)₂ per teaspoon, calculate the number of milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia. (1 tablespoon = 3 teaspoons.)Express the volume in milliliters to two significant figures.

We can establish the following relations:

1 tablespoon = 3 teaspoons
1 teaspoon contains 400 mg (0.400 g) of Mg(OH)₂
The molar mass of Mg(OH)₂ is 58.32 g/mol.
The molar ratio of HCl to Mg(OH)₂ is 2:1.
The concentration of HCl is 0.0324 mol/L.

The mililiters of HCl that neutralize 1 tablespoon of milf of magnesia are:

$1Tablespoon.\frac{3Teaspoon}{1Tablespoon} .\frac{0.400gMg(OH)_{2}}{1Teaspoon} .\frac{1molMg(OH)_{2}}{58.32gMg(OH)_{2}} .\frac{2molHCl}{1molMg(OH)_{2}} .\frac{1000mLHCl}{0.0324molHCl} =1.3 \times 10^{3} mLHCl$

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Jan Baptista van Helmont did an important experiment related to photosynthesis. He weighed a small willow tree and a pot of soil

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Answer:

Explanation:

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