Q3: The enthalpy of vaporization for water is: AHvop = + 44.0 kJ/mole Calculate the AH for evaporating 3.00 grams of water and AH for Condensing 20 grams of water.

Q: For many years drinking water has been cooled in hot climates by evaporating it from the surfaces of…

A: The heat released (q) in the evaporation of the given amount of water can be calculated by…

Q: If 0.40 kJ of heat is removed from a sample of water and it cools from 25°C to 15°C, what is the…

A: Mass of water is approximately 9.57 grams

Q: 23. Use the following information to determine the enthalpy for the reaction shown below. CS2(1) +…

A: C(graphite) + 2S(s) → CS2(l)                        Formation of CS2(l)= ∆H∘(CS2)= 87.9 kJ    CS2(l)…

Q: A 35.0-g sample of water at 25°C is mixed with 45.0 g of water at 88°C. Calculate the final…

A:

Q: Consider the combustion of liquid CH in oxygen gas to produce carbon dioxide gas and water vapor. In…

A:

Q: A 3.75 g piece of gold initially at 587.15 K is dropped into 20.6 mL of water at 295.75 K. Calculate…

A:

Q: A sample of solid lithium bromide and calcium chloride  were put in a lab for an hour. Their…

A: When 1 mol of a ionic substance is dissolve in water to form a solution at infinite dilution is…

Q: 22. Write a reaction that corresponds to the Suppose a 50.0 g block of silver (specific heat =…

A: The question is based on the law of conservation of energy. whatever heat lost by hot silver metal…

Q: Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water…

A: Convert 20 ounce of water into grams 1 ounce =28.3495 g 20 ounce = 566.99 g

Q: What quantity in moles of H₂ are required to give off 2501 kJ of heat in the following reaction? N₂…

A: The objective of the question is to find out the quantity in moles of H2 required to give off 2501…

Q: Duncan knows that it takes 36400 cal of energy to heat a pint of water from room temperature to…

A: for 1 pint of water energy absorbed = 36400cal 1 cal = 4.184 x 10 -3 kJ  so 36400 cal  = 36400 x…

Q: What would be the final temperature if 55.0g of H2O at 30 degrees C is added to 45.0g of H2O at 95…

A: The amount of energy for a particular amount of matter present at specific temperature with specific…

Q: How much heat is released when the temperature of an 8.21 g sample of gold decreases from 87.9 oC to…

A: q = mc∆T  q is the amount of heat energy released or absorbed m is the mass of substance  c is the…

Q: 1. In an experiment to determine the specific heat of copper, a piece of 50 gm copper is first…

A: Note: As per guidelines we can answer the first question, please post-second question separately…

Q: A common technique for forming metal electrodes on electronic devices is evaporation in a vacuum. In…

A: Given Data: The enthalpy of vaporization (ΔHvap) for gold = 310.9 kJ/mol given mass of  liquid gold…

Q: What is the amount of heat energy in joules required to raise the temperature of 10.00 g water…

A: The required relation is given below.

Q: For the chemical reaction H, (g) + F, (g) → 2 HF (g) AH° = -79.2 kJ/mol. What is the enthalpy (in…

A:

Q: A 27 g aluminum foil pan is used to roast vegetables.  The pan is put into a cold oven at 22 oC .…

A: The heat released or absorbed (q) by a substance when the temperature of that substance is raised is…

Q: A foundry worker places a 5.76 kg sheet of nickel at a temperature of 18°C on top of a 16.6 kg sheet…

A: The specific heat capacity for a given chemical substance or a solution refers to the amount of the…

Q: ow much heat is required to warm 1.20 Lof water from 20.0 ∘Cto 100.0 ∘C? (Assume a density of…

A: Amount of heat absorbed 'q 'to raise the temperature is found by the following equation,…

Q: How much energy (in calories) is required to melt 25.0 g of ice to water at 0.0 °C, heat the liquid…

A: Given that, heat of fusion of water = 79.7 cal g-1 To convert 25 g of ice at 0 ∘C to 25 g of water…

Q: A 100.0 g iron sample (specific heat 0.450 J/g K) at 100. deg C is added to 50.0 g for water at 26.5…

A: We know that, heat flows from higher temperature to the lower temperature. From the given…

Q: How many grams of water would require 2,247 joules of heat to raise its temperature from 36.86 °C to…

A: Solution - According to the question - Given - Given the heat of water = 2,247 joules change in…

Q: A 0.534 g sample of steam at 103.5 °C is condensed into a container with 4.98 g of water at 14.4 °C.…

A: Solutions                  Concept : Heat lost by steam = Heat gain by water

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.