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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 × 10^5 kg of HCN if the reaction has a 97.5% yield?

Solutions

Expert Solution

% yield = ( observed mass / therotical mass) x 100

97.5 = (1.5 x 105  / X) x 100

X = 153846.1 g

so therotical yield must be 153846.1 g g HCN

according to balanced reaction

2 x 27 g HCN require 2 x 17 g NH3

153846.1 g HCN require   153846.1 x 2 x 17 / 2 x 27 = 96866.0 g

mass of NH3 required = 96866.0 g

queen_honey_blossom answered 2 years ago
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