You start with 100mL of 14M HNO3 and 10grams of copper metal. How many moles of the nitrogen dioxide gas will be produced?

Chemistry

1 answer:

givi [52]2 years ago

7 0

Answer:

0.316 moles are produced.

Explanation:

We state the redox reaction:

4HNO₃ + Cu → Cu(NO₃)₂ + 2NO₂ + 2H₂O

We need to determine the limting reactant:

0.1 L . 14 M = 1.4 moles

10 g . 1mol/ 63.54g =0.158 mol

Cu is the limiting reactant. Let's see

4 moles of acid need 1 mol of Cu to react

1.4 moles of acid may react to (4 . 1) / 1.4 = 0.35 moles

We do not have enough Cu.

1 mol of Cu can produce 1 mol of NO₂

Then 0.158 moles will produce, 0.316 moles. (double of moles)

If we see stoichiometry, ratio is 1:2

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Given the balanced equation representing a reaction:

GrogVix [38]

As aluminium loses 12 moles of electrons oxygen gain 12 moles of electrons.

Explanation
4Al + 3 O2→ Al2O3
first write the ions of Aluminium and oxygen

that is, Aluminium ion is = Al^3+
oxygen ion is = O^2-
therefore one atom of Al loses 3 electrons moles while
one atom of O gain 2 electrons moles

from equation above there a total of number of Al atom are 4 =( 1 x4=4) atoms while
Oxygen atoms are 6= ( 3 x2=6) atoms

therefore the total number of Moles of Al lost is = 3 x 4 = 12 moles of electrons

total number of moles of O gained = 2 x6 = 12 moles of electrons

6 0

3 years ago

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Damm [24]

Explanation:

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Given that:

Element A has 3 valence electrons and element B has 2 valence electrons. To find the ionic compound, the valency of the cations and the anions are interchanged and are written in subscripts. Thus,

A B

3 2

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