Nitrogen and hydrogen gases react to form ammonia gas as follows: N_2(g) + 3 H_2

Question

Nitrogen and hydrogen gases react to form ammonia gas as follows: N_2(g) + 3 H_2(g) rightarrow 2 NH_3 (g) At a certain temperature and pressure, 1.2 L of N_2 reacts with 3.6 L of H_2. If all the N_2 and H_2 are consumed, what volume of NH_3, at the same temperature and pressure, will be produced? (a) What conditions are represented by the abbreviation STP? (b) What is the molar volume of an ideal gas at STP? (c) Room temperature is often assumed to be 25 degree C. Calculate the molar volume of an ideal gas at 25 degree C and 1 atm pressure. (d) If you measure pressure in bars instead of atmospheres, calculate the corresponding value of R in L-bar/mol-K.

Explanation / Answer

4. According to Gay-Lussac's law

Ratio of Volume = 1:3:2

So, Volume of N2=1.2L, H2= 3.6L so volume of NH3= 2.4L

5. a.STP = Standard Temperature and Pressure,

b. molar volume at STP= 22.414L

c. V = nRT/P = 1 x 0.082057 x 298.15 / 1 = 24.465 L

d. 8.3144598×102 L bar K1 mol1

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