Question

Provided all the informations to answer questions 11,12 a,b,c

Please I'm struggling what to write need help on these questions!!

Part B: Quantitatitve Analysis of the Dissolution of Anhydrous Magnesiu 6 Using weighing paper as shown, weigh out a 3-8 gram sample of magnesium sulfate on the analytica Record the exact mass to the 0.0001g Using a 7 Suspend a 0.1°C thermometer into a polystyrene cup so that it is about ½ inch from the bottom recording volumetric pipet, add 100.0 mL (using a 50.0 mL pipet twice) of deionized water and stir while time versus temperature data in 30 second intervals. After about 4 minutes add the magnesium continuous mixing while continuing to record data. Time/Temperature data should be collected for uip t minutes after the magnesium sulfate has dissolved. The temperature should level off and you should co minimum of five temperature readings AFTER the temperature has stabilized. (The more data you have the better your graphs will be.) sulfate with 8 Repeat step 7 a second time with a different amount of magnesium sulfate. Insert data into the appropriate number of tables in your notebook like the ones below 9 Collect rwo other sets of data from TWO other groups. Record them into your notebook. See the sample data tables below. Sample Data Tables Run 1 Run Run 3 Run 4 Mass of Mgso,(9) Volume of water (mL) Run 1 Time (sec) Temp (C) 30 60 etc.

Answer 1

11. The overall generalization of the dissolution of magnesium sulfate is that looking at the temperature trend one can realise that it is an exothermic reaction where there is release of heat which in turn results in the increasing trend of temperature.

12. A) Lattice energy is defined as the heat of formation for ions of opposite charge in the gas phase to combine into an ionic solid. Alternatively, it can be defined as the amount of heat energy required to break away the ions from ionic solid to a gas phase.

B) The amount of heat released when bonds are formed between ions and water molecules is called enthalpy of hydration.

C) The answer to the this part can be answered by the flowchart:

The heat of solution is the enthalpy change associated with the dissolution of a certain amount of solute in a given amount of solvent.

When a compound such as MgSO₄ dissolves in water the Mg²⁺ and SO_4^2- ions break away from the crystal lattice and enter the aqueous phase where they are surrounded by water molecules.

First, the lattice is broken up and the ions enter the gaseous phase.

MgSO₄(s) ----> Mg²⁺(g) + SO_4^2-(g)

The energy change for this process is called the the lattice energy, U.

Second, the gaseous Mg²⁺ and SO_4^2- ions enter the aqueous phase, where they are hydrated. During hydration, Mg²⁺and SO_4^2- ions are surrounded by H2O molecules which in turn results in heat release (enthalpy of hydration).

Mg²⁺(g) + SO₄^2-(g) ----> Mg²⁺(aq) + SO_4^2-(aq)

According to Hess's law, the overall energy change for the two steps will be the heat of solution

Hsoln = U + Hhydr