If 1.40 grams of nitrogen is used in the reaction, how many grams of hydrogen will be needed?
What's the reaction?
To determine how many grams of hydrogen are needed in the reaction, we need to know the balanced chemical equation for the reaction involving nitrogen and hydrogen. Once we have that, we can use stoichiometry to calculate the required quantity of hydrogen.
Let's assume that the balanced chemical equation for the reaction is:
N₂ + xH₂ → NH₃
In this equation, x represents the coefficient of H₂, which tells us the stoichiometric ratio between nitrogen and hydrogen. To balance the equation, we need to find the value of x.
Since we're given that 1.40 grams of nitrogen (N₂) is used in the reaction, we can convert this mass to moles using the molar mass of nitrogen, which is approximately 28.02 grams/mole.
Moles of nitrogen = Mass of nitrogen / Molar mass of nitrogen
Moles of nitrogen = 1.40 grams / 28.02 grams/mole ≈ 0.05 moles of nitrogen
According to the balanced equation, the stoichiometric ratio between nitrogen and hydrogen is 1:1. Therefore, the number of moles of hydrogen required is also approximately 0.05 moles.
Now, to find the mass of hydrogen, we need to convert moles to grams using the molar mass of hydrogen, which is approximately 2.02 grams/mole.
Mass of hydrogen = Moles of hydrogen × Molar mass of hydrogen
Mass of hydrogen = 0.05 moles × 2.02 grams/mole ≈ 0.10 grams of hydrogen
Therefore, approximately 0.10 grams of hydrogen will be needed in the reaction.
Note: The actual balanced chemical equation and stoichiometry values may vary depending on the specific reaction being referred to.