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kotegsom [21]
3 years ago
11

You wish to set up an electrochemical cell that has a copper anode and an

Chemistry
1 answer:
professor190 [17]3 years ago
4 0
I think cathode should be silver or gold
you can use silver nitrate solution or mercury nitrate solution
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Calculate the standard reaction enthalpy for the reaction NO2(g) → NO(g) + O(g) given +142.7 kJ/mol for the standard enthalpy of
bulgar [2K]

Answer:

The standard reaction enthalpy for the given reaction is 235.15 kJ/mol.

Explanation:

O_2(g) \rightarrow \frac{2}{3}O_3(g),\Delta H^o_{1}=142.7 kJ/mol..[1]

O_2(g) \rightarrow 2 O(g),\Delta H^o_{2}=498.4 kJ/mol..[2]

NO(g) + O_3(g)\rightarrow NO_2(g) + O_2(g) ,\Delta H^o_{3} = -200 kJ/mol..[3]

NO_2(g)\rightarrow NO(g) + O(g),\Delta H^o_{4}=?..[4]

Using Hess's law:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

2 × [4] = [2]- (3 ) × [1] - (2) × [3]

2\times \Delta H^o_{4}=\Delta H^o_{2} -3\times \Delta H^o_{1}-2\times \Delta H^o_{3}

2\times \Delta H^o_{4}=498.4 kJ/mol-3\times 142.7 kJ/mol-2\times -200 kJ/mol

2\times \Delta H^o_{4}=470.3 kJ/mol

\Delta H^o_{4}=\frac{470.3 kJ/mol}{2}=235.15 kJ/mol

The standard reaction enthalpy for the given reaction is 235.15 kJ/mol.

7 0
3 years ago
Question:<br> What is protecting us from the solar wind?
ale4655 [162]

Answer:

The magnetic field

Explanation:

5 0
2 years ago
Which of the following properties can be
Aleonysh [2.5K]

Answer:

Ability to conduct electricity

Melting point

4 0
3 years ago
The following reaction shows the products when sulfuric acid and aluminum hydroxide react.
scoray [572]

Leftover: approximately 11.73 g of sulfuric acid.

<h3>Explanation</h3>

Which reactant is <em>in excess</em>?

The theoretical yield of water from Al(OH)₃ is lower than that from H₂SO₄. As a  result,

  • Al(OH)₃ is the limiting reactant.
  • H₂SO₄ is in excess.

How many <em>moles</em> of H₂SO₄ is consumed?

Balanced equation:

2 Al(OH)₃ + 3 H₂SO₄ → Al₂(SO₄)₃ + 6 H₂O

Each mole of Al(OH)₃ corresponds to 3/2 moles of H₂SO4. The formula mass of Al(OH)₃ is 78.003 g/mol. There are 15 / 78.003 = 0.19230 moles of Al(OH)₃ in the five grams of Al(OH)₃ available. Al(OH)₃ is in excess, meaning that all 0.19230 moles will be consumed. Accordingly, 0.19230 × 3/2 = 0.28845 moles of H₂SO₄ will be consumed.

How many <em>grams</em> of H₂SO₄ is consumed?

The molar mass of H₂SO₄ is 98.076 g.mol. The mass of 0.28845 moles of H₂SO₄ is 0.28845 × 98.076 = 28.289 g.

How many <em>grams</em> of H₂SO₄ is in excess?

40 grams of sulfuric acid H₂SO₄ is available. 28.289 grams is consumed. The remaining 40 - 28.289 = 11.711 g is in excess. That's closest to the first option: 11.73 g of sulfuric acid.

6 0
3 years ago
What is the volume in ML
BabaBlast [244]

Answer:1 mL

Explanation:

4 0
3 years ago
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