This question is about the Haber process: N2(g) + 3H2(g) ⇌ 2NH3(g) The forward reaction is exothermic. 120 moles of hydrogen gas are mixed with 40.0 moles of nitrogen gas and pressurised. The mixture of gases is passed over an iron catalyst at 450 °C until the mixture reaches equilibrium. 20.0% of the reactants are converted to ammonia. The total volume of the mixture is 1.00 dm3.
a How many moles of nitrogen and of hydrogen remain at equilibrium? [2] b How many moles of ammonia are formed? [1]
My working 20/100 × 160 = 32 32 moles of ammonia are formed N2 H2 NH3 Initial moles 40 120 0 Change -x -3x +2x At equilbrium 40-x 120-3x 32 So x is 16 Im getting H2 72 moles and N2 24
This question is about the Haber process: N2(g) + 3H2(g) ⇌ 2NH3(g) The forward reaction is exothermic. 120 moles of hydrogen gas are mixed with 40.0 moles of nitrogen gas and pressurised. The mixture of gases is passed over an iron catalyst at 450 °C until the mixture reaches equilibrium. 20.0% of the reactants are converted to ammonia. The total volume of the mixture is 1.00 dm3.
a How many moles of nitrogen and of hydrogen remain at equilibrium? [2] b How many moles of ammonia are formed? [1]
My working 20/100 × 160 = 32 32 moles of ammonia are formed N2 H2 NH3 Initial moles 40 120 0 Change -x -3x +2x At equilbrium 40-x 120-3x 32 So x is 16 Im getting H2 72 moles and N2 24
The RIGHT ANSWERS ARE H2 96 N2 32
WHATS WRONG WITH MY WORKING??
Find the 20% for the nitrogen and the hydrogen moles separately, this would give you the correct answer.
Whats wrong with my ice tablee? Why isnt the answer coming through that method?
No idea tbh but why did you not just take the 32 divide it by 4 as 1 N and 3 H and subtract that number (8) from the nitrogen moles and from the hydrogen moles.