Question

Can you please show how to do the calculations I sent for run 2.

al values ofc where the o the maximum ot minim changes? lluirate by ggh ily gven by the oquatice lcrmining the transinoal f inflection poses change abe famly to see whas shand oonal value of c at whi unges. Try to discover i a have discoveed anomials given by the oqu Er what values of c does Exp Background Information We A chemical reaction involves breaking, making, or changing chemical bonds. These alterations in bonding lead to a change in enthalpy, AH, between the products and reactants. This enthalpy change takes into account the change in internal energy in the system and the work done by the system on ies surroundings during the reaction. If the reaction occurs at a constant pressure and in an adiabatic apparatus (no heat can leave or enter), the change in enthalpy will be equal to the heat absorbed or evolved, reflected by the temperature of the system decreasing or increasing, respectively. The heat of a reaction is determined in the laboratory by measuring this temperature change in a calorimeter. If you know the amount of heat required to change the temperature of the calorimeter, reactants, and products, you can calculate the heat of reaction or the enthalpy change. Pa nts? asimom pnnts of ever sarabola y 1- hola and several memb I. momials given by dhe co For what values of c a minimum poines wsimam poims of every wrve y-xx ustr eral members of the fr Calorimetry is used for many real-world applications. For example, the caloric content of any food, which appears on its nutritional label, is determined by calorimetry! A constant-volume, or "bomb," calorimeter is used to essentially burn the food completely, while the change in the temperature of water surrounding the reaction chamber is measured. This change in temperature is then used to calculate how much energy was released by the combustion reaction. A whole lot of chemistry goes into creating those nutritional labels! In this experiment you will measure the heat evolved in the reaction of magnesium with hydro- chloric acid. eme values have p = to minimize costs e. Fermat's Princir In this section we s minimizing dista Mg(s) +2H (aq)Mg(aq) + H,(g) In order to calculate the heat of this reaction very precisely, you would need to know the heat ca- pacities (heat required to change the temperature of one gram by one degree Celsius) of everything that changes temperature during the reaction, and the magnitudes of corrections for the amount of heat lost to the surroundings and for the heat produced by the mechanical stirring of the contents of the calorimeter. To simplify the calculations in this experiment, we will assume that the reactants will not change temperature during the reaction, as they will be consumed quickly, and that the heat absorbed by the hydrogen gas formed will be too small to add appreciably to the other terms. The corrections for heat loss and the other factors related to the apparatus will be included in one term, which we will call the heat capacity of the calorimeter. Ren to convert the o the function that orinciples discusse em carefully until are the given qu ram and identify In this experiment, your calorimeter will consist of two Styrofoam cups nested together. You will determine a value for the heat capacity of your calorimeter by studying a system for which the heat of reaction is known: the formation of water from its ions in dilute solution o he maximized or xy) for oche It may help to use eight, r for time. AH -57.320 Joules H (aq) +OH (aq)-H,O(aq) 68 Experiment 11

Answer 1

Run 2.

Mass of NaCl solution (m) = (50+56) mL * 1.04 g/mL = 110.24 g

The amount of heat produced from HCl-NaOH reaction (q) = m.C.$\Delta$T

Where 'C' is the specific heat of solution = 3.93 J/g.^oC

$\Delta$T is the change in temperature = 32.5 - 20 = 12.5 ^oC

i.e. q = 110.24 g * 3.93 J/g.^oC * 12.5 ^oC = 5415.54 J

Moles of water formed in the reaction (n) = moles of NaCl = 110.24 g/58.5 g.mol^-1 = 1.884 mol

Therefore, the enthalpy change ($\Delta$H) = q/n = 5415.54 J/1.884 = 2874.5 J