Given that 1 g of hydrogen combines completely with 8 g of oxygen to form water, how much water can you make with 10 g of hydrogen and 24 g of oxygen?
I got it!
24/8=3
24+3=27
To determine how much water can be formed with the given amounts of hydrogen and oxygen, we need to use the concept of the molar ratio. The molar ratio tells us the proportion in which elements combine in a chemical reaction.
1. Calculate the number of moles of hydrogen and oxygen:
Moles of hydrogen = mass of hydrogen (in this case, 10 g) / molar mass of hydrogen
= 10 g / 1 g/mol (molar mass of hydrogen)
= 10 mol
Moles of oxygen = mass of oxygen (in this case, 24 g) / molar mass of oxygen
= 24 g / 16 g/mol (molar mass of oxygen)
= 1.5 mol
2. Determine the limiting reactant: The limiting reactant is the reactant that is completely consumed in a chemical reaction. It determines the maximum amount of product that can be formed. To find the limiting reactant, we compare the moles of hydrogen and oxygen present:
Hydrogen: 10 mol
Oxygen: 1.5 mol
Since the ratio of hydrogen to oxygen required for water is 1:8, we can see that 1.5 moles of oxygen can react with 1.5 / 8 = 0.1875 moles of hydrogen. This means that the oxygen is in excess and hydrogen is the limiting reactant.
3. Calculate the amount of water formed using the stoichiometry of the balanced equation:
From the balanced equation, we know that 1 mole of hydrogen reacts with 8 moles of oxygen to form 9 moles of water.
Number of moles of water formed = moles of hydrogen (limiting reactant) * (moles of water / moles of hydrogen)
= 10 mol * (9 mol water / 1 mol hydrogen)
= 90 mol
4. Calculate the mass of water formed using the molar mass of water:
Mass of water formed = number of moles of water formed * molar mass of water
= 90 mol * 18 g/mol (molar mass of water)
= 1620 g
Therefore, 10 g of hydrogen and 24 g of oxygen can make 1620 g (or 1.62 kg) of water.