CH_4(g) + 2 Cl2(g) rightarrow CH_2Cl_2l(g) + 2 HCI(g) Use the following data to
ID: 530156 • Letter: C
Question
CH_4(g) + 2 Cl2(g) rightarrow CH_2Cl_2l(g) + 2 HCI(g) Use the following data to calculate delta H degree for the reaction: CH_4(g) + CI_2C(g) rightarrow CH_3Cl(g) + HCI(g), delta H degree = -983 kJ CH_3CI(g) + Cl_2(g) rightarrow CH_2CI_2(g) + HCI(g), delta h degree = -104 kJ Up to 10 points can be added to your score if you answer Q. 11 correctly: When 25.0 mL of 1.00, M HCI is added to 25.0 mL of 1.00 M NaOH at 25 00 degree Cin a calorimeter, the temperature of the solution increased to 27.50 degree C. Calculate delta H for the rea in kJ/moL. Assume that the specific heat of the solution is 4.18 J/(g degree C) density 1.00 g/mL, a that the heat capacity of the calorimeter = 0.Explanation / Answer
Ans On adding Equation 1 and 2, We get the main reaction and hence
Delta H = H1 + H2
= -98.3 + (-104)
= - 202.3 KJ