At a certain temperature, 0.4011 mol of N2 and 1.561 mol of H2 are placed in a 4.50 L container. N2(g)+3H2(g)↽−−⇀2NH3(g)

At equilibrium, 0.1601 mol of N2 is present. Calculate the equilibrium constant, kc=

Enzyme make a hormone as a catalyst

7is b8 is d9 is c10 is a11 is d

I'm sorry but i'm only grade

Answerδh > 0explanationc₆h₆  (s)  → c₆h₆ (l)if you are changing it from a solid to a liquid, you are pretty much melting the solid. this requires heat energy. therefore, the reaction is endothermic (takes in energy); the system enthalpy increases as the reaction proceeds: δh > 0.