One mol of any gas at STP occupies a volume of ___ L. How do you write this as a

Question

One mol of any gas at STP occupies a volume of ___ L. How do you write this as a conversion factor? For the following reaction: N_2(g) + 3H_2 (g) rightarrow 2NH_3(g) a. What volume of nitrogen at STP would be required to react with 0.100 mol of hydrogen? b. What volume of nitrogen at STP required to react with 0.100 g of hydrogen to produce ammonia? For the following reaction: N_2(g) + 3H_2 (g) rightarrow 2NH_3(g) c. What volume of nitrogen at 215 degree C and 715 mmHg would be required to react with 0.100 mol of hydrogen? d. What volume of nitrogen at 215 degree C and 4.56 atm would be required to produce 75.3 g of ammonia?

Explanation / Answer

1 Mole of any gas at STP occupies 22.4 L of volume.

(a) One mole of N2 will react with 3 moles of hydrogen to form ammonia.

Volume of N2 at STP = 22.4 L

Volume of N2 at STP to react with 0.100 of H2 = (0.100 mol /3 mol) x 22.4

= 0.747 L

(b) Moles = mass/molar mass

No. of moles of H2 = 0.100/2 = 0.05 moles

One mole of N2 will react with 3 moles of hydrogen to form ammonia.

Volume of N2 at STP = 22.4 L

Volume of N2 = (0.05 mol /3 mol) x 22.4 = 0.373 L

(c) One mole of N2 will react with 3 moles of hydrogen to form ammonia. So,

Moles of N2 = 0.100/3 = 0.0333

Volume of nitrogen needed can be calculated from PV=nRT,

V = nRT/P

= 2.21 x 0.082057 x 488.15 K / 0.941 atm

= 1.42 L

(d) moles NH3 needed = mass / molar mass

= 75.3/17.034

= 4.42 moles

1 Mole of nitrogen forms 2 moles NH3

So for the formation of ammonia half mole of N2 is needed, i.e, 2.21 moles.

Volume of nitrogen needed can be calculated from PV=nRT,

V = nRT/P

= 2.21 x 0.082057 x 488.15 K / 4.56 atm

= 19.4 L

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