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Calculate the standard enthalpy of forma...

Calculate the standard enthalpy of formation of `CH_(3)OH(l)` from the following data
`CH_(3)OH(i)+(3)/(2)O_(2)(g)rarrCO_(2)(g)+2H_(2)O(1), Delta_(r)H^(Ө)=-726 kJmol^(-1)`
C(graphite) `+O_(2)(g)rarrCO_(2)(g),Delta_(c)H^(Ө)=-393 kJ mol^(-1)`
`H_(2)(g)+(1)/(2)O_(2)(g)rarrH_(2)O(1),Delta(f)H^(Ө) =-286kJ mol^(-1)`

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Verified by Experts

`C(s)+2H_(2)(g)+1/2O_(2)(g)rarr CH_(3)OH(l), Delta_(f)H^(Θ)=`?
Equation (ii) `+2xx"Equation"` (iii) -Equation (i) gives the required equation with
`DeltaH=-393+2(-286)-(-726)kJ "mol"^(-1)=-239 kJ "mol"^(-1)`
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Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: CH_(3)OH(l)+3/2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l), …(i), Delta_(r)H_(1)^(Θ)=-726 kJ mol^(-1) C(g)+O_(2)(g) rarr CO_(2)(g), …(ii), Delta_(c )H_(2)^(Θ)=-393 kJ mol^(-1) H_(2)(g)+1/2O_(2)(g) rarr H_(2)O(l), ...(iii), Delta_(f)H_(3)^(Θ)=-286 kJ mol^(-1)

Methanol can be prepared synthetically by heating carbon monoxide and hydrogen gases under pressure in the presence of a catalyst. The reaction is CO(g) +2H_(2)(g) rarr CH_(3)OH(l) Determine the enthalpy of this reaction by an appropriate combinantion of the following data: a. C_(("graphite")) +(1)/(2)O_(2)(g) rarr CO(g), DeltaH^(Theta)=- 110.5kJ mol^(-1) b. C_(("graphite")) +O_(2)(g) rarr CO_(2)(g), DeltaH^(Theta) =- 393.5 kJ mol^(-1) c. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(l), DeltaH^(Theta) =- 285.9kJ mol^(-1) d. CH_(3)OH(l) +(3)/(2)O_(2)(g)rarr CO_(2)(g) +2H_(2)O(l),DeltaH^(Theta) =- 726.6 kJ mol^(-1)

Calculate enthalpy of formation of methane (CH_4) from the following data : (i) C(s) + O_(2)(g) to CO_(2) (g) , Delta_rH^(@) = -393.5 KJ mol^(-1) (ii) H_2(g) + 1/2 O_(2)(g) to H_(2)O(l) , Deta_r H^(@) = -285.5 kJ mol^(-1) (iii) CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l), Delta_(r)H^(@) = -890.3 kJ mol^(-1) .

Calculate the heat of formation of n butane from the following data: a. 2C_(4)H_(10)(g) +13O_(2)(g) rarr 8CO_(2)(g) +10H_(2)O(l), DeltaH = - 5757.2 kJ b. C(s) +O_(2) (g)rarrCO_(2)(g), DeltaH =- 405.4 kJ c. 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l), DeltaH =- 572.4 kJ

Calculate the heat of formation of n butane from the followinf data: a. 2C_(4)H_(10)(g) +13O_(2)(g) rarr 8CO_(2)(g) +10H_(2)O(l), DeltaH = - 5757.2 kJ b. C(s) +O_(2) (g)rarrCO_(2)(g), DeltaH =- 405.4 kJ c. 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l), DeltaH =- 572.4 kJ

With the help of thermochemical equations given below, determine Delta_(r )H^(Θ) at 298 K for the following reaction: C("graphite")+2H_(2)(g) rarr CH_(4)(g),Delta_(r )H^(Θ) = ? C("graphite")+O_(2)(g) rarr CH_(2)(g), Delta_(r )H^(Θ) = -393.5 kJ mol^(-1) ...(1) H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l) , Delta_(r )H^(Θ) = -285.8 kJ mol^(-1) ...(2) CO_2(2)(g)+2H_(2)O(l) rarr CH_(4)(g)+2O_(2)(g) , Delta_(r )H^(Θ) = +890.3 kJ mol^(-1) ...(3)

Calculate the enthalpy of formation of Delta_(f)H for C_(2)H_(5)OH from tabulated data and its heat of combustion as represented by the following equaitons: i. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g), DeltaH^(Theta) =- 241.8 kJ mol^(-1) ii. C(s) +O_(2)(g) rarr CO_(2)(g),DeltaH^(Theta) =- 393.5kJ mol^(-1) iii. C_(2)H_(5)OH (l) +3O_(2)(g) rarr 3H_(2)O(g) + 2CO_(2)(g), DeltaH^(Theta) =- 1234.7kJ mol^(-1)

Compounds with carbon-carbon double bond, such as ethylene, C_(2)H_(4) , add hydrogen in a reaction called hydrogenation. C_(2)H_(4)(g)+H_(2)(g) rarr C_(2)H_(6)(g) Calculate enthalpy change for the reaction, using the following combustion data C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(g) , Delta_("comb")H^(Θ) = -1401 kJ mol^(-1) C_(2)H_(6)(g) + 7//2O_(2)(g)rarr 2CO_(2) (g) + 3H_(2)O(l) , Delta_("comb")H^(Θ) = -1550kJ H_(2)(g) + 1//2O_(2)(g) rarr H_(2)O(l) , Delta_("comb")H^(Θ) = -286.0 kJ mol^(-1)

Calculate the heat of formation of methanol (CH_3OH) from thhe following data: CH_3OH(l) + 3/2O_2(g) to CO_2(g) + 2H_2O (l),Delta =-726 kJ C(s) + O_2(g) to CO_2(g) , DeltaH = -394 kJ H_2(g) + 1/2 O_2(g) to H_2O(l) , Delta H = -286 kJ

Calculate the standard heat of formation of C_2H_5OH(l) from the following data: (a) C_2H_5OH (l) + 2O_2(g) to 2CO_2(g) + 3H_2O (l) , DeltaH^@ = - 1366.5 kJ (b) Delta_f H^@ [ CO_2] = -393.5 kJ mol^(-1), Delta_f H^@ [ H_2O(l)] = -285.5 kJ mol^(-1) .

CENGAGE CHEMISTRY ENGLISH-NCERT BASED EXERCISE-Thermodynamics
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