Organic Chemistry Answers

List down the different types of hydrocarbons, explaining the types of reactions it undergoes, each with an example. 

Explain the working principle of constant volume and constant pressure calorimeters

An experiment to measure the enthalpy change for the reaction of aqueous copper(II) sulfate, CuSO4(aq) and zinc, Zn(s) was carried out in a coffee cup calorimeter as follows. Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq)

50.0 cm3 of 1.00 mol dm–3 copper(II) sulfate solution was placed in a polystyrene cup and its average temperature after three readings was noted to be 25OC and the zinc powder was added . The final temperature was noted to be 91.5 OC. Calulate the heat of the reaction in kJ 

The standard enthalpy change of three combustion reactions is given below in kJ. 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) ∆HO = –3120

2H2(g) + O2(g) → 2H2O(l) ∆HO = –572

C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) ΔHO = –1411

Based on the above information, calculate the standard change in enthalpy, ∆HO, for the following reaction. C2H6(g) → C2H4(g) + H2(g) 

The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25C of 1.8 x 10-5. The reaction is as follows : CH3COOH (aq)  CH3COO- (aq) + H+ (aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO- is 8.1 x 10-3 moles in the same 0.500 L, calculate [H+] for the reaction. 

Complete the following acid base reactions, indicate the conjugate acid-base pairs, and state whether the reaction has a large or small equilibrium constant.

a. CH3COOH(aq) + NH3(aq) 

b. H2CO3 (aq) + NO3 - (aq) 

c. H2CO3 (aq) + H2O (l) 

d. HCO3 - (aq) + H2O (l) 

e. NH3 (aq) + H2O (l) 