Question

How many grams of H, would be formed if 34 grams of carbon reacted with an unlimited amount of H₂O? The reaction

is:

C + H₂O → CO + H₂

The atomic mass of C is 12.01 g/mole. The atomic mass of H2 is 2.016 g/mole. Finish the problem by choosing the correct format for dimensional analysis.

Answer 1

To determine the number of grams of hydrogen (H) formed if 34 grams of carbon react with an unlimited amount of H₂O, we can use stoichiometry. 2.831 mol of carbon will produce 5.70 g of H₂.

Step-by-step explanation:

To determine the number of grams of hydrogen (H) formed if 34 grams of carbon react with an unlimited amount of H₂O, we need to use stoichiometry. The balanced chemical equation is C + H₂O → CO + H₂. From the equation, we can see that for every mole of carbon, one mole of CO and one mole of H₂ are formed. The molar mass of carbon is 12.01 g/mol and the molar mass of H₂ is 2.016 g/mol.

First, we need to convert the mass of carbon to moles using its molar mass:

34 g C * (1 mol C / 12.01 g C) = 2.831 mol C

Since the ratio of carbon to hydrogen is 1:1, 2.831 mol of carbon will produce 2.831 mol of H₂. To convert these moles of H₂ to grams, we can use the molar mass of H₂:

2.831 mol H₂ * (2.016 g H₂ / 1 mol H₂) = 5.70 g H₂