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meriva
3 years ago
5

Write a balanced half-reaction describing the oxidation of solid chromium to aqueous chromium(IV) cations.

Chemistry
1 answer:
Pachacha [2.7K]3 years ago
7 0

Answer:

Cr(s) ⟶ Cr⁴⁺(aq) + 4e⁻  

Explanation:

1. Write the skeleton half-reaction

Cr(s) ⟶ Cr⁴⁺(aq)

2. Balance charge

Add electrons to the side that needs them.

You have 4+ on the right and 0 on the left. You must add 4e⁻ to the right to balance the charge.

Cr(s) ⟶ Cr⁴⁺(aq) + 4e⁻

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What is he empirical formula for the compound that is of 1.85 moles of nitrogen and 4.63 miles of oxygen
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The empirical formula is N₂O₅.

The empirical formula is the <em>simplest whole-number ratio of atoms</em> in a compound.  

The ratio of atoms is the same as the ratio of moles, so our job is to calculate the <em>molar ratio of N:O</em>.  

I like to summarize the calculations in a table.  

<u>Element</u> <u>Moles</u>  <u>Ratio¹ </u>  <u> ×2²  </u>  <u>Integers</u>³

     N        1.85    1             2             2

     O        4.63    2.503   5.005     5

¹To get the molar ratio, you divide each number of moles by the smallest number (1.85).

²Multiply these values by a number (2) that makes the numbers in the ratio close to integers.

³Round off the number in the ratio to integers (2 and 5).

The empirical formula is N₂O₅.

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Determine the enthalpy change when 23.5 g of carbon is reacted with oxygen according to the reaction C(s) + O2(g) CO2(g) delta H
xeze [42]
We are provided with the amount of energy released when one mole of carbon reacts. We mus first convert the given mass of carbon to moles and then compute the energy released for the given amount.

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1.96 moles will release:
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The enthalpy change of the reaction will be -772.24 kJ
8 0
3 years ago
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