(a) 71.2°C (b) 63.6°C (c) 51.0°C (d) 42.0°C (e) 69.5°C 5. Calculate the energy i
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(a) 71.2°C (b) 63.6°C (c) 51.0°C (d) 42.0°C (e) 69.5°C 5. Calculate the energy in the form of heat (in kJ) required to convert 100.0 grams of liquid water at 80.0°C to steam at 122°C. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion 333 J/g; heat of vaporization 2256 J/8; specific heat capacities: liquid water 4.184 J/g.K, steam 1.92 J/gK) (a) 238 kJ (b) 226 kJ (c) 4.22 kJ (d) 8.37 k.J (e) 17.6 kJ 6. The molar heat capacity of gaseous hexane at 25.0° C is 198 J/mol.°C. What is its specific heat? (a) 17.1x10 J/(gC) (b) 171 J/(g. C) (c) 2.30 J/(g °C) (d) 229 J/(g C) (e) 1.71x104 J/(g C 7. The thermochemical equation for the combustion of butane is shown below. 13 mol- rxn What is the enthalpy change for the following reaction? 8 CO2(g) + 10H20(g)--2 C4H,o(g) + i30,(g) (a) +1439 k.J/mol-rxn (b) +2877 kJ/mol-rxn (c) 5754 kJ/mol-rxn (d) 2877 kJ/mol-rxnExplanation / Answer
6) Molar heat Capacity is an energy required to raise one mole of the molecule by one degree Celsius.
as we know
Specific heat = molar heat capacity/molar mass
molar mass of hexane =86.18g
specific heat= 86.18*198=17063.64J/g oC=17*103J/g oC
7) As we know, On reversing the equation, enthalpy of reaction become negative of enthalpy of that equation,
Enthalpy of the reverse equation is positive of given enthalpy but the required equation is multiplied by coefficient 2 so, Overall,
Enthalpy of 8CO2(g) +10H2O(g) - 2C2H4(g) + 13O2(g) = 2*2877KJ/mol=5754kJ/mol
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