8. The heat of neutralization of sulphuric acid by sodium hydroxide is -55.84 kJ/mole of water produced. In a calorimeter, 50.0 mL of a 1.05 M NaOH solution was mixed with 25.0 ml of a 1.86 M sulphuric acid solution. Initally both solutions were at the same temperature, 24.72 °C. The two solutions were mixed. Determine the final temperature of the mixture. Assume the specific heat of the solution to be 3.89 J/g °C and the density of the solution to be 1.02 grams/cm³. Assume a perfect system and no energy is lost to the surroundings. Hint: this is a limiting reactant problem.

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Q: When 1.31 g of KClO3 was added to 138.34 g of water in a calorimeter, the  temperature dropped by…

A: mass of KCIO3 = 1.31 g mass of water = 138.34 g Temperature dropped = 0.506 °C Heat capacity of H2O…

Q: When a 7.00 g sample of KCN is dissolved in water in a calorimeter that has a total heat capacity of…

A:

Q: 5. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water…

A: Mass of metal =59.047 g Mass of water = 100g ( density of water is1g/ml)

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A:

Q: 5.00 – mL of 0.64M HCl and 45.00 – mL 0.77M NaOH, both initially at 26.0°C, are mixed in a…

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Q: When 21.0 g of 0.200 M NaCl(ag) at 18.7 °C is added to 18.0 g of 0.100 M AgNO3(aq) at 18.7°C in a…

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Q: A cold pack contains 134.4 g of water and 40.7 g of ammonium nitrate. What will be the final…

A: The formula which is used in the solution is shown below. Q = mcΔT ⇒ ΔT = Q/mc

Q: What is the heat of a reaction, in joules, with a total reaction mixture volume of 57.1 mL if the…

A: Heat capacity: The amount of heat required to increase the temperature of one gram of a substance by…

Q: A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in…

A: The required equation is given below.

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A: Mass of the colarado oil = 4.1 g

Q: 48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction…

A: Given: Volume of HCl solution = 48.2 mL = 0.0482 L                               (Since 1 L = 1000…

Q: When 6.30 g sample of solid potassium hydroxide (MM= 56.11g/mol) is dissolved in 101.00 g of water…

A: Given, mass of sample of sodium potassium hydroxide = 6.30 g mass of water = 101.00 g Initial…

Q: The enthalpy change when a strong acid is neutralized by strong base is –56.1 kJ/mol.  If 12.0 mL of…

A: Given : concentration of HBr = 6 M and volume of HBr solution = 12 mL = 0.012 L…

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Q: What is the specific heat of 85,885.86 mL of a substance, that has a recorded temperature of 429.2…

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.