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The reaction for the industrial production of hydrogen cyanide is given below. 2CH4 + 2NH3 +...

The reaction for the industrial production of hydrogen cyanide is given below.

2CH4 + 2NH3 + 3O2 --> 2HCN + 6H2O

What mass of NH3 is required for the synthesis of 1.5 × 105 kg of HCN if the reaction has a 97.5% yield?

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Expert Solution

The reaction for the industrial production of hydrogen cyanide is given below.

2CH4 + 2NH3 + 3O2 --> 2HCN + 6H2O

What mass of NH3 is required for the synthesis of 1.5 × 105 kg of HCN if the reaction has a 97.5% yield?

First calculate the moles of HCN:

1.5*10^5 kg *1000g / 1.0 kg / molar mass HCN, 27.0253 g / mole

= 5550354.668 moles HCN

Now, calculate the moles of NH3 as follows:

5550354.668 moles HCN * 2 mole NH3/ 2 mole HCN

= 5550354.668 moles NH3

Amount of NH3 = Number of moles * molar mass

= 5550354.668 moles NH3 * 17.031 g / mole

= 9.45*10^7 g

= 9.45*10^4 kg NH3

Here the reaction the reaction has a 97.5%

So, 9.45*10^4 kg NH3 / 0.975= 9.695*10^4 kg NH3

queen_honey_blossom answered 2 years ago
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