The next three questions pertain to the complete combustion ofethyl acetate unde

Question

The next three questions pertain to the complete combustion ofethyl acetate under constant pressure: CH3COOC2H5(l) + 5O2(g) ®4CO2(g) + 4H2O(l)    H= -2238.1 kJ/mol How much heat is given off during the reaction, per mole of carbondioxide produHow much heat is given off when25.9 g of ethyl acetate is burned in excessoxygen?
The burning ethyl acetatefrom the previous question is used to heat 5.1 L of water at22.5°C. What would be the final temperature of the water?Assume all the heat produced in the last question is absorbed bythe water. Enter your answer in degrees Celsius, withoutunits.
The density of water at 22.5°C is 1.00 g/mL. At thistemperature range, the average specific heat of water is 4.18J/(g·K).
CH3COOC2H5(l) + 5O2(g) ®4CO2(g) + 4H2O(l)    H= -2238.1 kJ/mol The density of water at 22.5°C is 1.00 g/mL. At thistemperature range, the average specific heat of water is 4.18J/(g·K).

Explanation / Answer

molar mass ethyl acetate = 88.1 g/mol 25.9 g ethyl acetate *( 1 mol/88.1 g)*(2238.1 kJ/mol) = 657.965834~ 658 kJ b) T = Q/[m*Cp] = 658 kJ *1e3 J/1kJ / [ 5.1 L*(1000g /1L) * 4.18 J/g/C] T = 30.8643322 C Tfinal = Tinit + T = 22.5 + 30.9 = 53.4 C

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.