Question

Prelab questions 1. What is the significance of the statement "qsystem + Surroundings zero Law of Thermodynamics"? statement "qsystem + Surroundings = zero" in relation to the First 2. A student measured heat of neutralization in a Styrofoam "Coffee Cup calorimeter by mixing 25.0 mL of 1.0 M NaOH solution with 250 mL of 10 M HCI solution. Write the balanced equation and identify the limiting reactant in this experiment. If heat of this exothermic reaction was determined to be found -1295 J, what is the heat of neutralization in kJ/mole? 3. There are three approaches to determine enthalpy changes in a process. One can do direct orimetric measurement or one can use Hess's Law or standard enthalpy of formation. AH! Write net ionic equation for neutralization equation for neutralization of strong base (e.g., NaOH(aq)) and strong acid (e.g., Estimate AHneutralization using AH' values for H (aq), OH (aq) and H O () textbook as 0, -230.0 and -285.83 kJ/mole, respectively.

Answer 1

1) This means that entropy is a conserved measure, that is, what is produced by entropy in a system is obtained from another side, in this case from the surroundings.

2) The reaction that occurs is:

NaOH + HCl = NaCl + H2O

Both reagents are limits because they have the same amount of moles and the same stoichiometric coefficient, the moles are:

n = M * V = 1 M * 0.025 L = 0.025 mol

Enthalpy change is calculated:

ΔH = - q / n = 1,295 kJ / 0.025 = 51.8 kJ / mol

3) The NIE that occurs is:

H + + OH- = H2O

The enthalpy change is:

ΔH = ΔHf products - ΔHf reagents = - 285.83 - 0 + 230 = - 55.83 kJ / mol

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