How do I solve the last question using all the information above?

. . . ........ (b) A student carried out an experiment to determine the enthalpy change of combustion of pentan-1-ol, CH3(CH2)4OH. In the experiment 1.76g of pentan-1-ol) was burnt. The energy was used to heat 250 cm3) of water from 24.0 .C to 78.0 .C. 78- 24= 54 (i) Calculate the energy released, in KJ, during combustion of 1.76 g pentan-1-ol. The specific heat capacity of water = 4.18Jg-1K-1.-4.18 Density of water = 1.00gcm 3.. # 1000 2509 5 0.25 kg ( kg ) (OC ) = MCAT = 0.25 X 4180 x 64 = 564305 + 1000 = 56. 435 ks. 56.43 energy = ................. . .. ... ............ KJ [1] (ii) Calculate the amount, in moles, of pentan-1-ol that was burnt. 1176 = 0102 mol CH3 ( CH2) 4 OH mr -(12x5) + (12)+ 8% 16 = 88 amount = ..........9....Q.............. ............ mol [2] (iii) Calculate the enthalpy change of combustion of pentan-1-ol. Give your answer to three significant figures. AH= .. ............... KJmoll [3]