How will an increase in pressure affect the following equilibrium? CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH...
How will an increase in pressure affect the following equilibrium? CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH = −176 kJ
Shift toward products. Shift toward reactants. No change. Explain?
Homework Answers
Solid and liquid substances
are not affected by change in pressure since they are not involved
in equilibrium constant expression Kp because partial pressure of
solids and liquids is considered 1.
On increasing the pressure , volume decreases and number of moles increases , since reactant side has 1 gaseous mole and product side side has no gaseous moles. Equilibrium shifts in such a way so as to decrease moles of CO2. Hence equilibrium shifts toward products.
Shifts toward products.
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How will an increase in pressure affect the
following equilibrium? CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH...
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e. -1135 Given the following reactions: CaCO3 (s)-> Cao (s) + CO2 (g) C (s, graphite) + O2 (g)-> Co2 (g) AH-393.5 kJ the enthalpy of the reaction CaCO3 (s) -> CaO (s) + C (s, graphite) + O2 (g) ΔH = 178.1 kJ is kJ Select one: 4 a. 7.01 x 10 b. 571.6 ) c. 215.4 d. -215.4 ie. -571.6 Check Given the data in the table below, AH for the reaction
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