1. at 2257 K and 1.00 atm total pressure, water is 1.77 per cent decomposed at e
ID: 940494 • Letter: 1
Question
1. at 2257 K and 1.00 atm total pressure, water is 1.77 per cent decomposed at equilibrium
by way of the reaction 2 H20(g) = 2 H2(g) + 02(g). Calculate (a) K, (b) rG, and (c) rG at this
temperature.
2. on in the Data section. calculate the standard Gibbs energy and the
equilibrium constant at (a) 298 K and (b) 400 K for the reaction PbO(s) + CO(g) = Pb(s) + CO2(g).
Assume that the reaction enthalpy is independent of temperature.
3. Estimate the temperature at which CaC03(calcite) decomposes. The reaction is
CaCO3 (s) CaO(s) + CO2(g)
4. when ammonium nitrate undergoes decomposition, only gases are produced,
according to the equation
NH4NO3(s) N2O(g) + 2H2O(g)
What is the total volume of gases produced at 546 K and 1.00 atm pressure when 240 g of
ammonium nitrate ( F.W. NH4NO3 = 80) undergoes the above decomposition reaction.
ammonium nitrate ( F.W.
Explanation / Answer
3.
considering the following thermodynamic data
DeltaH] = 178.5 kJ/mol
DeltaS = 161.0 J/(mol*K)
we know that ,
dG = dH - T dS
for the reaction to occur spontaneously, dG = 0
therefore putting values, T = 1108.69 K
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