N2(g) + 3H2(g) 2NH3(g) at STP
How many litres of ammonia gas is produced using 5 litres of H2?
5L H2 x (2L NH3 / 3L H2) = 3.33L NH3
How many moles of N2 are needed?
5L H2 x (1L N2 / 3L H2) x (1 mol N2 / 22.41L N2@STP) = 0.0744 mole N2
22.4 liters/mol
3.33 L NH3/ (2 Liters NH3/1 liter N2) = 1.67 L N2
1.67 L * 1 mol.22.4 L = .0743 check agree :)
looks good
you might want to be aware of significant figures
thank you!
9. We want to produce 2.75 mol of NH 3 . How many moles of nitrogen would be required N 2 + 3H 2 2NH 3
To calculate the number of liters of ammonia gas produced using 5 liters of H2, you can start with the given amount of H2 and use the stoichiometry of the reaction. Looking at the balanced chemical equation, you can see that for every 3 moles of H2, you get 2 moles of NH3.
Using the conversion factor of 2L NH3 / 3L H2 (from the stoichiometry), you can set up the following equation:
5L H2 x (2L NH3 / 3L H2) = 3.33L NH3
By canceling out the units of liters of H2, you are left with the volume of NH3, which is 3.33 liters.
To calculate the number of moles of N2 needed for the reaction, you can use a similar approach. From the balanced chemical equation, you can see that for every 1 mole of N2, you need 3 moles of H2.
Using the conversion factors of 1L N2 / 3L H2 and 1 mol N2 / 22.41L N2@STP (where 22.41L is the molar volume of an ideal gas at standard temperature and pressure), you can set up the following equation:
5L H2 x (1L N2 / 3L H2) x (1 mol N2 / 22.41L N2@STP) = 0.0744 mole N2
By canceling out the units of liters of H2, you are left with the number of moles of N2, which is 0.0744 mole.