digitalwwnorton.com/15197 ult 52% 11/02/17 lp This is a Numeric Entry question/I

Question

digitalwwnorton.com/15197 ult 52% 11/02/17 lp This is a Numeric Entry question/It is worth 1 point/You have unlimited attempts/ 13 Question ( point) a See page 236 1st attempt See Periodic Table The complete combustion of 1.05 g of cinnamaldeyde (CoHgO, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter 3.30 kJ/ C) produced an increase in temperature of 14.0 "C. Calculate the molar enthalpy of combustion of cinnamaldehyde (4Hcomb (in kilojoules per mole of cinnamaldehyde). KJ/mol be 13 OF 24 QUESTIONS COMPLETED here to search DOLL

Explanation / Answer

Given that;

Mass of cinnamaldehye ; C9H8O = 1.05 g

Temperature change = 14.0C

C calorimeter =3.30KJ/C

First calculate the total amount of heat = C calorimeter * Temperature change

= 3.30KJ/C *14.0C

=46.2 KJ

= 46200 J

Now calculate the mole of cinnamaldehye ; C9H8O in 1.05 g as follows:

Number of moles = 1.05 g/ molar mass; 132 g / mol

= 0.00795 moles

Now calculate the molar enthalpy by divide the number of mole sin total amount of heat as follows:

molar enthalpy = 46.2KJ /0.00795 moles

=5811.32 l KJ/ MOLE

Related Questions

Navigate

• Browse (All)
• Browse D
• Subjects

---

---

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