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aleksandr82 [10.1K]
3 years ago
11

An industrial manufacturer wants to convert 175 kg of methane into HCN. Calculate the masses of ammonia and molecular oxygen req

uired for this synthesis.
Chemistry
1 answer:
Tema [17]3 years ago
4 0
Given:

175 kilograms of Methane (CH4) to be synthesized into Hydrogen Cyanide (HCN)

The balanced chemical equation is shown below:

2 CH4<span> + 2 NH</span>3<span> + 3 O</span>2<span> → 2 HCN + 6 H</span>2<span>O
</span>
To calculate for the masses of ammonia and oxygen needed, our basis will be 175 kg CH4.

Molar mass:
CH4 = 16 kg/kmol
NH3 = 17 kg/kmol
O2 = 32 kg/kmol

mass of NH3 = 175 kg CH4 / 16 kg/kmol * (2/2) * 17 kg/kmol 
mass of NH3 = 185.94 kg NH3 needed

mass of O2 = 175 kg CH4 / 16 kg/kmol * (3/2) * 32 kg/kmol
mass of O2 = 525 kg

mass of O = 525 kg / 32 kg/kmol * (1/2) * 16 kg/kmol
mass of O = 131.25 kg O 
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We can also perform a similar calculation for the mass defect and binding energy for nuclear reactions using the masses of the a
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Answer:

See Explanation

Explanation:

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[235.04393 + 1.00867] - [ 136.92532 + 96.91095 + 2(1.00867)]

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0.19899 amu = 0.19899 * 1.66 * 10^-27 = 3.3 * 10^-28 Kg

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Hence the mass defect is;

[10.01294 + 1.00867] - [7.01600 + 4.00260]

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0.00301 amu = 0.00301 * 1.66 * 10^-27 = 4.997 * 10^-30 Kg

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7 0
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MULTIPLE CHOICE
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Answer:

its very simple ans we have 2 just multiply256

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Answer:

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Explanation:

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