Calculate the temperature (K) at which the equation as written is at equilibrium
ID: 893074 • Letter: C
Question
Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
CaO(s) + H2O(l) ? Ca(OH)2(s)
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At a temperature of 890 K the equation as written is at equilibrium. Determine the change in entropy (?S?) of reaction (J/K) at this temperature. Express your answer to three significant figures.
CCl4(l) ? CCl4(g)
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At a temperature of 298 K the equation as written is at equilibrium. Determine the change in enthalpy (?H?) of reaction (kJ) at this temperature. Express your answer to three significant figures.
MgCO3(s) ? MgO(s) + CO2(g)
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Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
I2(s) ? I2(g)
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Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
BaO(s) + CO2(g) ? BaCO3(s)
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At a temperature of 680 K the equation as written is at equilibrium. Determine the change in entropy (?S?) of reaction (J/K) at this temperature. Express your answer to three significant figures.
CaO(s) + H2O(l) ? Ca(OH)2(s)
Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
CaO(s) + H2O(l) ? Ca(OH)2(s)
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Formula Molar Mass (g/mol) ?G°f (kJ/mol) ?H°f (kJ/mol) S° (J/(K mol)) CCl4(l) 153.82 -68.6 -139 CCl4(g) 153.82 -53.7 -96 T = 890 K R = 8.314 J/(K mol)At a temperature of 890 K the equation as written is at equilibrium. Determine the change in entropy (?S?) of reaction (J/K) at this temperature. Express your answer to three significant figures.
CCl4(l) ? CCl4(g)
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Formula Molar Mass (g/mol) ?G°f (kJ/mol) ?H°f (kJ/mol) S° (J/(K mol)) MgCO3(s) 84.32 -1096 MgO(s) 40.30 -601.7 CO2(g) 44.01 -393.5 T = 298 K R = 8.314 J/(K mol)At a temperature of 298 K the equation as written is at equilibrium. Determine the change in enthalpy (?H?) of reaction (kJ) at this temperature. Express your answer to three significant figures.
MgCO3(s) ? MgO(s) + CO2(g)
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Formula Molar Mass (g/mol) ?G°f (kJ/mol) ?H°f (kJ/mol) S° (J/(K mol)) I2(s) 253.812 0 0 116.14 I2(g) 253.812 19.33 62.44 260.69 T = (NA) K R = 8.314 J/(K mol)Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
I2(s) ? I2(g)
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Formula Molar Mass (g/mol) ?G°f (kJ/mol) ?H°f (kJ/mol) S° (J/(K mol)) BaO(s) 153.32 -552.3 -582.0 70.3 CO2(g) 44.01 -394.4 -393.5 213.7 BaCO3(s) 197.34 -1138 -1216 112 T = (NA) K R = 8.314 J/(K mol)Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures.
BaO(s) + CO2(g) ? BaCO3(s)
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Formula Molar Mass (g/mol) ?G°f (kJ/mol) ?H°f (kJ/mol) S° (J/(K mol)) CaO(s) 56.077 -604.0 -635.1 H2O(l) 18.015 -237.13 -285.83 Ca(OH)2(s) 74.093 -898.6 -986.1 T = 680 K R = 8.314 J/(K mol)At a temperature of 680 K the equation as written is at equilibrium. Determine the change in entropy (?S?) of reaction (J/K) at this temperature. Express your answer to three significant figures.
CaO(s) + H2O(l) ? Ca(OH)2(s)
Explanation / Answer
CaO(s) + H2O(l) Ca(OH)2(s)
DATA:
CaO(s) 56.077 -604.0 -635.1 39.7
H2O(l) 18.015 -237.13 -285.83 69.91
Ca(OH)2(s) 74.093 -898.6 -986.1 83.4
NOTE that for an eqution to be in equilibrium
dG = 0
That is
dg = dH - T*dS = 0
dH and dS may be cnsidered independt of Temperature so we need to "modify" temperature in order to make this tru
dH - T*dS = 0
dH = TdS
CaO(s) + H2O(l) Ca(OH)2(s)
dH = Hproducts - Hreactants = -986.1 - (-635.1 + -285.83) = -65.17 kJ/mol
dS = Sproducts - Sreactants = 83.4 - (69.91+39.7) = -26.21 J/mol
Substitute
dH = TdS
-65.17*1000 =T*-26.21
T = -65170 /(-26.21) = 2486 K
T = 2486 K
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