equilbrium calculation (1 Viewer)

[zeee1999]

why am i getting this question wrong??

Solid ammonium hydrogen sulfide (NH4HS) decomposes to form ammonia gas and hydrogen sulfide gas (H2S). 2.00 moles of ammonium hydrogen sulfide were placed in a sealed 3.00 L container and the system was allowed to reach equilibrium. At
equilibrium, there were 0.0328 moles of ammonia gas. Calculate the equilibrium constant for this reaction

this is my working out
NH4HS NH3 H2S
initial 0.66 (2/3) 0 0

change - 0.0328 +0.0328 +0.0328


equilbrium 0.6272 0.0328 0.0328


k= [0.0328][0.0328]/[0.6272] k= 1.7x10-3

 

[same1111]

why am i getting this question wrong??

Solid ammonium hydrogen sulfide (NH4HS) decomposes to form ammonia gas and hydrogen sulfide gas (H2S). 2.00 moles of ammonium hydrogen sulfide were placed in a sealed 3.00 L container and the system was allowed to reach equilibrium. At
equilibrium, there were 0.0328 moles of ammonia gas. Calculate the equilibrium constant for this reaction

this is my working out
NH4HS NH3 H2S
initial 0.66 (2/3) 0 0

change - 0.0328 +0.0328 +0.0328


equilbrium 0.6272 0.0328 0.0328


k= [0.0328][0.0328]/[0.6272] k= 1.7x10-3

u dont include liquids or solids in the equillibrium constant expression. I havent checked ur table but if the table is correct then just remove the "solid hydrogen sulfide" from the equillibrium. Just use the two gases in to calculate the constant. If there is nothing on the bottom you put a "1". Should give you the right answer if the table is correct.