how many gram of h2 needed to react with 3.10 n2
To determine how many grams of H2 are needed to react with 3.10 moles of N2, we refer to the balanced chemical equation for the reaction between H2 and N2:
N2 + 3H2 -> 2NH3
From the equation, we can see that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.
Now we can set up a proportion to find the amount of H2 needed:
(3.10 moles N2) / (1 mole N2) = (x moles H2) / (3 moles H2)
Cross-multiplying, we get:
3.10 moles N2 * 3 moles H2 = x moles H2
9.30 moles H2 = x moles H2
So, 9.30 moles of H2 are needed to react with 3.10 moles of N2.
To convert moles to grams, we need to know the molar mass of H2, which is approximately 2 g/mol.
To calculate the mass, we use the formula:
mass = moles * molar mass
mass = 9.30 moles * 2 g/mol
mass = 18.6 grams
Therefore, approximately 18.6 grams of H2 are needed to react with 3.10 moles of N2.