What is the cquilibrium concentration of hcip the reaction is run at 25°c and all data is collected at 25°c. 12 h2g)cl2g 2 hcl(g) ag ,m= -6.38 k 0,40 0.050 initial, m 0.050 4+2k +2 x 0.21 m 603-xxufs) 05-y 0,48 m . d. 0.57 m -( -l0.38- .31 x1d ur (bbr -2h73p 4+2x 25x10 iv +v2 13 for the exothermic reaction in question #12, will it release heat energy or require heat energy as it reaches equilibrium? the initial concentrations are given below and the reaction is run at 25°c ag6.38 k h2( c 2 hclg) 0.050 0.40 initial, m 0.050 the reaction will require heat energy to reach equilibriutm. the reaction will release heat energy as it reaches cquilibrium. equilibrium. the reaction is c 8.3

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

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