2. a neutralization reaction was carried out in a calorimeter. the change in temperature (at) of the solution was 5.6 °c and the mass of the solution was 100.0 g. calculate the amount of heat energy gained by the solution (qsol). use 4.18 j/(g. c) as the specific heat, cs, of the solution.

3. what is the value of qreaction for the neutralization reaction described in number 2?

4. how many moles of phosphoric acid are contained in 50.0 ml of 0.60 m h3po4?

5. what is the value of ahr kj/mol phosphoric acid) if 50.0 ml of 0.60 m reaction in h3po4 was used in the reaction described in number 2?

Explanation:

2. First we have to calculate the heat gained by the solution.

where,

q = heat gained = ?

c = specific heat of solution =

m = Mass of the solution = 100.0 g

= final temperature

= initial temperature

ΔT = = 5.6°C

Now put all the given values in the above formula, we get:

The amount of heat energy gained by the solution 2,340.8 J.

3.

Heat gained by solution = Heat released on neutralization reaction

2,340.8 Joules is the value of reaction for the neutralization reaction described in number 2.

4.

Moles of phosphoric acid = n

Volume of the phosphoric acid solution = 50.0 mL = 0.050 L

Molarity of the phosphoric acid solution = 0.60 M

0.03 moles of phosphoric acid are contained in 50.0 mL of 0.60 M phosphoric acid solution.

5. To calculate the enthalpy change during the reaction.

where,

n = moles of phosphoric acid = 0.03 moles

= enthalpy change = ?

q = heat gained = 2,340.8 J = 2.3408 kJ

Therefore, the enthalpy change during the reaction is -78.027 kJ/mole

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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