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PIT_PIT [208]
3 years ago
7

How many moles of ammonia (nh3 will be produced from 4.0 moles of nitrogen (n2?

Chemistry
1 answer:
Lana71 [14]3 years ago
3 0
Standard equation would be N2(g)+3H2(g)==>2NH3(g), so through stoichiometry, (4 mol N2)(2mol NH3/1 mol N2), assuming excess H2, would yield 8 moles of NH3.  
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Which one of these is the accepted name for the compound n2o5?
Leya [2.2K]
C is the correct answer. For nonmetal-nonmetal compounds, use the Greek prefixes

Mono - 1
Di - 2
Tri - 3
Tetra - 4
Penta - 5
Hexa - 6
Hepta - 7

And so on...

The reason D is not right is because a and o cannot be next to each other in between prefix and element.

Hope this helps!

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The unbalanced equation for the reduction of copper(I) sulfide with oxygen is given below. What mass of copper is produced from
uranmaximum [27]

<u>Answer:</u> The mass of copper produced is 7.12 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

Given mass of copper (I) sulfide = 8.80 g

Molar mass of copper (I) sulfide = 156.2 g/mol

Putting values in equation 1, we get:

\text{Moles of copper (I) sulfide}=\frac{8.80g}{156.2g/mol}=0.056mol

The chemical equation for the reaction of copper (I) sulfide and oxygen gas follows:

Cu_2S+O_2\rightarrow 2Cu+SO_2

By Stoichiometry of the reaction:

1 mole of copper (I) sulfide produces 2 moles of copper

So, 0.056 moles of copper (I) sulfide will produce = \frac{2}{1}\times 0.056=0.112mol of copper

Now, calculating the mass of copper from equation 1, we get:

Molar mass of copper = 63.55 g/mol

Moles of copper = 0.112 moles

Putting values in equation 1, we get:

0.112mol=\frac{\text{Mass of copper}{63.55g/mol}\\\\\text{Mass of copper}=(0.112mol\times 63.55g/mol)=7.12g

Hence, the mass of copper produced is 7.12 grams

6 0
3 years ago
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