Calculate the standard enthalpy change, ΔH, for the formation of 1 mol of strontium carbonate (the material that gives the red color in fireworks) from its elements.
Sr(s) + C(graphite) + 32 O2(g) -----> SrCO3(s)
The information available is:
(1) Sr(s)+ 12O2(g) ---->SrO(s) DeltaH= -592kj
(2) SrO(s) + CO2(g) -----> SrCO3(s) DeltaH= -234kj
(3) C(graphite) + O2 (g) ----->CO2 (g) DeltaH= -394kl
The information available is:
(1) Sr(s)+ 12O2(g) ---->SrO(s) DeltaH= -592kj
(2) SrO(s) + CO2(g) -----> SrCO3(s) DeltaH= -234kj
(3) C(graphite) + O2 (g) ----->CO2 (g) DeltaH= -394k
The change in enthalpy of reaction can be obtained from Hess Law.
So we need to rearrange the above given equations so that we can obtain the desired equation No. 4.
(4) Sr(s) + C(graphite) + 32 O2(g) -----> SrCO3(s)
The equation (4) can be obtanied by adding the above three equations
Sr + 1/2O2 + SrO + CO2 + C + O2 ---> SrO + SrCO3 + CO2
cancel the common terms on the two side of equation
Sr+ 3/2 O2 + C --> SrCO3 ( Our desired equation )
So Enthapy of reaction = DeltaH1 + DeltaH2 + DeltaH3 = -592kj + (-234kj) + (-394kJ) = -1220 KJ / moles
Calculate the standard enthalpy change, ΔH, for the formation of 1 mol of strontium carbonate (the...
Use the following data to calculate the standard enthalpy of formation of solid strontium carbonate SrCO3 (s) → SrO (s) + CO2(s) ΔH° = 234 kJ/mol ΔHf° of CO2 (g) = -394 kJ/mol ΔHf° of SrO(s) = -592 kJ/mol A) -752 kJ B) 752 kJ C) -1220 kJ D) -1812 kJ E) 1812 kJ f) 1220
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