Question

For which reaction will kp = kc?

1) s(s) + o2(g) ⇌ so2(g)
2) 2 hgo(s) ⇌ hg(l) + o2(g)
3) caco3(s) ⇌ cao(s) + CO₂⁺(g)
4) h2co3(s) ⇌ h2o(l) + CO₂⁺(g)
5) 2 h2o(l) ⇌ 2 h2(g) + o2(g)

Answer 1

None of the reactions provided will have Kp equal to Kc, as they all involve a change in the number of moles of gaseous substances, violating the condition for Kp to be equal to Kc.

Step-by-step explanation:

For the reaction where Kp equals Kc, we need to have a reaction where the number of moles of gaseous reactants is equal to the number of moles of gaseous products. Given the equation for the equilibrium constant in terms of pressure (Kp) and concentration (Kc):

Kp = Kc(RT)^(Delta n)

where R is the universal gas constant, T is the temperature in Kelvin, and Delta n is the difference in moles of gaseous products and reactants. If Delta n is zero, which happens when the number of moles of gaseous products is equal to the number of moles of gaseous reactants, then Kp will equal Kc since (RT)^(0) is 1.

Looking at the provided options:

• Option 1) involves a solid and a gas forming a gas, and the moles don't cancel out.
• Option 2) also involves a phase change in addition to a gas being produced.
• Option 3), CaCO3(s) ⇌ CaO(s) + CO2(g), involves only a gaseous product with no gaseous reactants and can't be the answer.
• Option 4) has liquid and gaseous products forming from a solid, which won't make Kp equal Kc.
• Option 5) has two moles of liquid forming two moles of gas and one mole of a different gas, changing the number of moles in the phase we're interested in, thus Kp won't equal Kc.

None of the reactions provided will have Kp equal to Kc as they all involve a change in the number of moles of gaseous substances.