Follow the description of the reaction below and answer the question following it:
In a dry cell battery the reaction that releases energy is: metallic zinc reacts with ammonium chloride to form zinc (II) chloride and ammonia (NH3) and Hydrogen gas.
a. Write a balanced equation for the reaction.
b. What is the ratio of number of moles of ammonia produced: number of moles of zinc consumed?
c. Calculate the mass of ammonia released when 32.84 g of Zinc are consumed
2007-11-12 20:03:44 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Zn 2NH4Cl ----->ZnCl2 + 2NH3 + H2
2:1
Zn = 65.4
NH3 = 17.0
32.84/65.4 * 17.0 = 8.54g
2:1 ratio 2*8.54 = 17.08g
17.08g of ammonia is produced
2007-11-12 20:17:32 · answer #1 · answered by science_guy 5 · 0⤊ 0⤋
Ammonium chloride is NH4Cl
Zinc chloride is ZnCl2
The (balanced) reaction is then
Zn + 2NH4Cl ----> ZnCl2 + 2NH3 + H2^
Count up the atoms of each element on each side:
Zn = 1
Cl = 2
N = 2
H = 8
to check that it is balanced
The right side shows 2NH3, while the left has only one Zn, so the ratio of moles NH3 to Zn is 2:1
The atomic mass of Zn is 65.4 g/mole, so 32.84 g of Zn is 32.84/65.4 = 0.502 mole; using the ratio above, 2X this is the moles of Ammonia, or 1.00 moles. The molecular mass of NH3 is 17.0, so the mass of ammonia is 1.0*17.0 = 17 grams
2007-11-12 20:21:05 · answer #2 · answered by gp4rts 7 · 0⤊ 0⤋
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2016-05-22 22:28:54 · answer #3 · answered by ? 3 · 0⤊ 0⤋
Any formula there?
2007-11-12 20:06:16 · answer #4 · answered by Anonymous · 0⤊ 0⤋