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mars1129 [50]
3 years ago
7

Calculate the standard enthalpy change for the reaction at 25 ∘ C. Standard enthalpy of formation values can be found in this li

st of thermodynamic properties. C3H8(g)+ 5O2(g) ⟶ 3CO2(g)+ 4H2O(g)
Chemistry
1 answer:
meriva3 years ago
4 0

Answer:

The standard enthalpy change for the reaction at 25^{0}\textrm{C} is -2043.999kJ

Explanation:

Standard enthalpy change (\Delta H_{rxn}^{0}) for the given reaction is expressed as:

\Delta H_{rxn}^{0}=[3mol\times \Delta H_{f}^{0}(CO_{2})_{g}]+[4mol\times \Delta H_{f}^{0}(H_{2}O)_{g}]-[1mol\times \Delta H_{f}^{0}(C_{3}H_{8})_{g}]-[5mol\times \Delta H_{f}^{0}(O_{2})_{g}]

Where \Delta H_{f}^{0} refers standard enthalpy of formation

Plug in all the given values from literature in the above equation:

\Delta H_{rxn}^{0}=[3mol\times (-393.509kJ/mol)]+[4mol\times (-241.818kJ/mol)]-[1mol\times (-103.8kJ/mol)]-[5mol\times (0kJ/mol)]=-2043.999kJ

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Cyclohexane has a freezing point of 6.50 ∘C and a Kf of 20.0 ∘C/m. What is the freezing point of a solution made by dissolving 0
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Explanation:

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T_f^0-T_f=i\times k_f\times \frac{w_2\times 1000}{M_2\times w_1}

where,

T_f = freezing point of solution = ?

T^o_f =  freezing point of solvent (cyclohexane) = 6.50^oC

k_f =  freezing point constant  of  solvent (cyclohexane)  = 20.0^oC/m

m = molality

i = Van't Hoff factor = 1 (for non-electrolyte)

w_2 = mass of solute (biphenyl) = 0.771 g

w_1 = mass of solvent (cyclohexane) = 25.0 g

M_2 = molar mass of solute (biphenyl) =

Now put all the given values in the above formula, we get:

(6.50-T_f)^oC=1\times (20.0^oC/m)\times \frac{(0.771g)\times 1000}{154\times (25.0g)}

(6.50-T_f)^oC=4.01

T_f=2.49^0C

Therefore, the freezing point of a solution made by dissolving 0.771 g of biphenyl in 25.0 g of cyclohexane is 2.49^0C

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