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4 years ago

The standard free energy change for a reaction can be calculated using the equation

Chemistry

1 answer:

snow_lady [41]4 years ago

7 0

Answer:

a) 1,737 kJ

b) -1,93 kJ

Explanation:

The standard free energy change (ΔG) can be determined using:

ΔG = -nFE

a) For the reaction:

Fumarate²⁻ + CoQH₂ ⇄ succinate²⁻ + CoQ

The transferred electrons are 2, As E=-0,009V:

ΔG = -2×96,5kJ/molV×-0,009V

ΔG = 1,737 kJ

b) For the reaction:

cytc1 (Fe²⁺) + cytc (Fe³⁺) ⇄ cytc1 (Fe³⁺) + cytc (Fe²⁺)

The transferred electron is n=1 and E=0,02V:

ΔG = -1×96,5kJ/molV×0,02V

ΔG = -1,93 kJ

I hope it helps!

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Is caesium a solid liquid or gas

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Answer:

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Explanation:

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3 years ago

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Arisa [49]

1. Given the following equation: N2 (g) + 3 H2 (g) ↔ 2NH3 (g) ΔH = -92 kJ/mol

a. this reaction is exothermic as ΔH is -ve

b. the equilibrium will shift 2 the left if nitrogen gas is removed

c. the equilibrium shift 2 the right if the temperature is lowered

d. the equilibrium shift 2 the left if ammonia (NH3) is added

e. principle of thermodynamic potential or Gibbs energy is used to answer B-D

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3 years ago

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Describe the redox reaction. Check all that apply 2AI(s) + 3ZnCI2(g) → 3Zn(s) + 2AICI3(aq).

Inga [223]

Answer:

Zinc is reduced.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

Explanation:

For the reaction:

2AI(s) + 3ZnCI₂(g) → 3Zn(s) + 2AICI₃(aq).

For the elements in the reactants side:

Al has (0) oxidation state and converted to (+3) oxidation state in the products (AlCl₃), which means Al is oxidized and it is the reducing agent.

So, we can check that: Aluminum is oxidized.

Zn has the oxidation state (+2) in the reactants side (ZnCl₂) and converted to (0) in the products side (Zn), which means that Zn is reduced and it is the oxidizing agent.

So, we can check that: Zinc is reduced.

and can not check: Zinc is the reducing agent.

The oxidation state of Cl does not change, it is the same in both sides (-1).

So, we can check: The oxidation number of chlorine does not change.

and can not check: Aluminum atoms transfer electrons to chlorine atoms.

So, the choices will be:

Zinc is reduced.

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Aluminum is oxidized.

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4 years ago

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A student must use 220 mL of hot water in a lab procedure. Calculate the amount of heat required to raise the temperature of 220

Inessa [10]

Answer:

64,433.6 Joules

Explanation:

We are given;

Volume of water as 220 mL
Initial temperature as 30°C
Final temperature as 100°C
Specific heat capacity of water as 4.184 J/g°C

We are required to calculate the amount of heat required to raise the temperature.

We know that amount of heat is calculated by;

Q = mcΔT , where m is the mass, c is the specific heat, ΔT is the change in temperature.

Density of water is 1 g/mL

Thus, mass of water is 220 g

ΔT = 100°C - 30°C

= 70°C

Therefore;

Amount of heat, Q = 220g × 4.184 J/g°C × 70°C

= 64,433.6 Joules

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3 years ago

If you remove two protons and two neutrons from a gold atom (au), what new element is formed (if any)?

ivanzaharov [21]

Answer: Iridium

Explanation:

The atomic number of Iridium is 77.

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2 years ago