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Lyrx [107]
3 years ago
8

Given the following balanced reaction: 2 NH3 +CO2 --> CH4N2O + H2O A reaction produces 87.5g of CH4N2O upon the reaction of 6

8.2g of NH3 with 105 g of CO2. (a) determine the limiting reagent. (b) Theoretical yield of CH4N2O (c) percent yield of the reaction (d) show full work and explain in your own words how you solved this problem.
(a,b,c,d are all different parts to the question)
Chemistry
1 answer:
tankabanditka [31]3 years ago
5 0

Answer:

ml lang yan pre tara laro

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239 L

Explanation:

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C_3H_8 (g) + O_2 (g)\rightarrow CO_2 (g) + H_2O (l)

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C_3H_8 (g) + O_2 (g)\rightarrow 3 CO_2 (g) + H_2O (l)

Secondly, 8 hydrogens in total (4 water molecules) are required on the right:

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On the right, we have a total of 10 oxygen atoms, this implies we need 5 oxygen molecules on the left:

C_3H_8 (g) + 5 O_2 (g)\rightarrow 3 CO_2 (g) + 4 H_2O (l)

2. Calculate moles of propane using the the ratio of mass to molar mass:

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According to the stoichiometry, we have 3 times greater amount of carbon dioxide:

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Use the ideal gas law to solve for volume:

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Marina86 [1]

Answer:

Two unlike charged ions.

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The positive charge on one and the negative on the other helps form the ionic bond.

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