A.)the equilibrium constant, kp, for the following reaction is 0.110 at 298 k:
nh4hs(s) nh3(g) + h2s(g)
calculate the equilibrium partial pressure of h2s when 0.371 moles of nh4hs(s) is introduced into a 1.00 l vessel at 298 k.
ph2s = ? ? atm
b.) the equilibrium constant, kp, for the following reaction is 0.497 at 500 k:
pcl5(g) pcl3(g) + cl2(g)
calculate the equilibrium partial pressures of all species when pcl5(g) is introduced into an evacuated flask at a pressure of 1.47 atm at 500 k .
ppcl5 = ? ? atm
ppcl3 = ? ? atm
pcl2 = ? ? atm

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

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