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) ÎrGΦ, and (c) ÎrG 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) ï CaO(s) + CO2(g)
4. when ammonium nitrate undergoes decomposition, only gases are produced,
according to the equation
NH4NO3(s) ï 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.
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) ÎrGΦ, and (c) ÎrG 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) ï CaO(s) + CO2(g)
4. when ammonium nitrate undergoes decomposition, only gases are produced,
according to the equation
NH4NO3(s) ï 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.
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