The industrial synthesis of methanol, CH₃OH, is catalyzed by metal oxides. Billions of kg are produced annually for use in polymers and fuel additives.
CO + 2 H₂ $\rarr$ CH₃OH
How many kg of hydrogen will be required to produce 1.0 x 10⁵ kg of methanol?

Question

The industrial synthesis of methanol, CH₃OH, is catalyzed by metal oxides. Billions of kg are produced annually for use in polymers and fuel additives.
CO + 2 H₂

\rarr

CH₃OH
How many kg of hydrogen will be required to produce 1.0 x 10⁵ kg of methanol?

Quizplus · Accepted Answer

To produce 1.0 x 10^5 kg of methanol, we need to calculate the amount of hydrogen required. The molar mass of methanol (CH3OH) is 32 g/mol, and the molar mass of hydrogen (H2) is 2 g/mol. The reaction shows that 2 moles of H2 are needed for each mole of methanol. Therefore, for 1.0 x 10^5 kg (or 1.0 x 10^8 g) of methanol, we need (1.0 x 10^8 g / 32 g/mol) x 2 mol H2 x 2 g/mol = 1.25 x 10^4 kg of H2, which is approximately 1.3 x 10^4 kg.

The Industrial Synthesis of Methanol, CH3OH, Is Catalyzed by Metal →\rarr→

The Industrial Synthesis of Methanol, CH₃OH, Is Catalyzed by Metal $\rarr$