How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimited amount of H2O? The reaction is:
C + H2O → CO + H2
Is this equation balanced?
Obviously the equation is balanced.
Each mole of C produces 1 mole of H2.
How many moles of C in 34g?
That's how many moles of H2 you get.
Convert that back to grams.
You'll get (34/12) * 2 grams
To determine the number of grams of H2 formed when 34 grams of carbon reacts with an unlimited amount of H2O, we first need to determine the limiting reactant and then use stoichiometry to calculate the amount of H2 produced.
1. Start by balancing the chemical equation:
C + H2O → CO + H2
To balance the equation, we need to ensure that the same number of each element is present on both sides of the equation.
The balanced equation is:
C + 2H2O → CO + 2H2
2. Calculate the molar mass of carbon (C), hydrogen (H2), and water (H2O).
- Molar mass of C = 12.01 g/mol
- Molar mass of H2 = 2.02 g/mol
- Molar mass of H2O = 18.02 g/mol
3. Use the molar mass and molar ratio in the balanced equation to determine the number of moles of carbon (C) present in 34 grams.
- Number of moles of C = mass of C / molar mass of C
- Number of moles of C = 34 g / 12.01 g/mol
4. Use the balanced equation to determine the number of moles of H2 produced.
From the balanced equation, we see that each mole of carbon (C) reacts with 2 moles of H2, as the stoichiometric coefficient is 2. Therefore, the molar ratio of H2 to C is 2:1.
- Number of moles of H2 = Number of moles of C / 2
5. Calculate the mass of H2 formed from the number of moles of H2.
- Mass of H2 = Number of moles of H2 × molar mass of H2
By following these steps, you can determine the amount of H2 formed when 34 grams of carbon reacts with an unlimited amount of H2O.