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The value of ##K_P## is 0.2.
1. Calculate mass of NH₄I reacted.
You started with 5 g of NH₄I and ended up with 2.56 g at equilibrium. So
Mass of NH₄I reacted = 5 g – 2.56 g = 2.4 g (1 significant figure + 1 guard digit.
2. Calculate moles of NH₃ and HI formed.
NH₄I(s) ⇌ NH₃(g) + HI(g)
Moles of NH₃ formed = ##2.4″ g NH”_4″I” × (“1 mol NH”_4″I”)/(“144.94 g NH”_4″I”) × (“1 mol NH”_3)/(“1 mol NH”_4″I”) = “0.017 mol NH”_3##
Moles of HI formed = ##”0.017 mol NH”_3 × “1 mol HI”/(“1 mol NH”_3) =
“0.017 mol HI”##
3. Calculate partial pressures of NH₃ and of HI.
##PV = nRT##
##P_”NH₃” = P_”HI” = (nRT)/V = (“0.017 mol” × “0.0821 L·atm·K”^-1″mol”^-1 × “676 K”)/”2.00 L”## = 0.47 atm
4. Calculate ##K_P##.
##K_P = P_”NH₃”P_”HI”## = 0.47 × 0.47 = 0.2
Note: The answer can have only 1 significant figure, because that is all you gave for the starting mass of NH₄I. If you need more precision, you will have to recalculate.
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