Question

In the harber-bosch process, the reactant nitrogen is drawn from the air while the hydrogen is produced by burning methane gas (CH4) in a series of processes that can be simplified as: CH4 + 2H2O —> CO2 + 4H2 3a. A small ammonia plant used 123,000 g of H2 gas per day. Determine the mass of CO2 (in g) that will be released as the H2 is produced. Show all work

Answer 1

Answer:Main Answer:

The mass of CO2 released in the production of 123,000 g of H2 gas is 265,200 g.

Explanation: From the given equation, we can see that the production of 4 moles of H2 requires the combustion of 1 mole of CH4, resulting in the release of 2 moles of H2O and 1 mole of CO2. The molar mass of H2 is 2 g/mol, and the molar mass of CO2 is 44 g/mol. Therefore, the mass of CO2 released in the production of 123,000 g of H2 is (123,000/2) x (1/4) x 44 = 265,200 g.