The following reaction consumes 2.15 kg of CO(g): CO(g) + H2O(g) --> CO2(g) + H2(g) How many total liters of gas are formed if the products are collected at STP?

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To determine the total liters of gas formed, we need to calculate the number of moles of CO2 and H2 produced in the reaction.

First, let's convert the mass of CO consumed to moles. The molar mass of CO is 28.01 g/mol.

Moles of CO = mass of CO / molar mass of CO
= 2.15 kg / 28.01 g/mol
= 76.691 mol

According to the balanced equation, the stoichiometric ratio of CO2 to CO is 1:1, and the stoichiometric ratio of H2 to CO is also 1:1.

Therefore, the moles of CO2 produced = 76.691 mol
and the moles of H2 produced = 76.691 mol

At STP (Standard Temperature and Pressure), the molar volume of any ideal gas is 22.4 L/mol.

So, the total liters of gas formed = (moles of CO2 + moles of H2) * molar volume
= (76.691 mol + 76.691 mol) * 22.4 L/mol
= 3422.9864 L

Therefore, approximately 3422.99 liters of gas are formed if the products are collected at STP.