Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.

Q: 1. Ethanol has a heat of vaporization of +841 J/g when it transitions from liquid to gas What is the…

A: Heat of vaporization is defined as the energy change when one mole of a liquid is converted to one…

Q: • If you boil water on a stove, the temperature of the water will remain close to 100 °C. As long as…

A: Boiling point is defined as the temperature at which a substance changes from liquid phase to gas…

Q: The heat capacity of liquid ethanol is 2.45 J/g-deg C. How much heat do you need to add to 100 g of…

A: Given: Specific heat capacity of ethanol = 2.45 J/g⋅ oC Mass of ethanol = 100.0 g Initial…

Q: How much heat is transferred from a 4.10 g gold nugget (specific heat = 0.129 J/g-°C) initially at…

A:

Q: How much energy is needed to heat 356 g of ice at -10 °C to 0 °C and melt it?Heat =…

A: Heat capacity is calculated by below equation,

Q: What amount of heat energy is needed to warm 4.00 grams of H2O (ℓ) by 25°C?

A: Specific heat is the amount of heat energy required to raise the temperature of substance by 1°C ,…

Q: What quantity of heat (in kJ) will be absorbed by a 47.1 g piece of aluminum (specific heat = 0.930…

A:

Q: How much heat (in kJ) will be absorbed by a 79.1 g piece of aluminum (specific heat = 0.930 J/g･°C)…

A: Given: Mass of Al piece = 79.1 gSpecific heat of Al = 0.930 J/g.°CInitial temperature = 23.0 °CFinal…

Q: How much heat (in J) is evolved or absorbed when a 36.2 g sample of aluminum (specific heat = 0.900…

A: In this question gven data , m=36.2gheat capacity=0.900J/(g K)∆T =T2 -T1T2=87.5°C=273+87.5=360.5KT1…

Q: Calculate the enthalpy change when 245g of ice melts.

A: melting of ice is known as fusion of water.

Q: Calculate the energy absorbed/released, in kJ, when 12.72 g of liquid water is turned to ice. Be…

A: In liquid state water molecules have less intermolecular forces of attraction compare to solid.

Q: How much heat, in kJ, will be absorbed by a 25.0 g piece of aluminum (specific heat = 0.930 J/g.°C)…

A: Mass of aluminium = 25.0 g Specific heat of the system(C) = 0.93 J/g 0C Initial temperature = 25 0C…

Q: Sweat cools the body because evaporation is an endothermic process H2O(l) → H2O(g)         ∆H ̊ =…

A: Given mass = 135 lbs ΔT = 3.65°C c = 4J/g°C ΔH = 44.01 kJ/mol

Q: 6. A container of yogurt has 240 Calories. What mass of perspiration would someone have to lose to…

A: Given that, a container of yogurt has 240 calories. At body temperature, the latent heat of…

Q: How much heat (in J) is evolved or absorbed when a 35.1 g sample of ethanol (specific heat = 2.46…

A: specific heat capacity is the amount of heat required to raise the temperature of 1 Kg of a…

Q: Which of the following are equal to the specific heat of water? Select all that apply. 4.184 J/g°C…

A: The heat energy absorbed or evolved during the reaction is calculated by using specific heat…

Q: 1.82 Benzene (C,H6) is an organic liquid that freezes at 5.5 °C (see Figure 11.15) to form…

A: Given, Temperature = 5.5°C Mass = 15.5 g Enthalpy Change of fusion = 9.95 kJ mol-1

Q: How much heat is required to convert solid ice with a mass of 960 g at a temperature of -10.0 °C to…

A: Heat in kilojoules can be calculated using the specific heat capacity, temperature difference and…

Q: What is the final temperature when a 5.0 g sample of brass initially at 25 oC absorbs 75 J of heat?…

A:

Q: How much heat is required to raise the temperature of 789g of liquid ammonia, form 25°C to 82.2°C?

A: Given: The mass of liquid ammonia is 789 g. The initial temperature is 25oC. The final temperature…

Q: How much heat energy is needed to warm 50.0 g of carbon (specific heat = 0.71 J/g ºC) from 25 ºC to…

A:

Q: How much heat is absorbed when 25.0g of water warms from 10.2oC to 38.0oC

A: According to calorimetry,  q = m × c × ∆T Where q = heat released or heat absorbed,   c = specific…

Q: How much energy is needed to raise the temperature of 80.0 g of water from 22.0 oC to 76.0 oC?  The…

A: The energy required for increasing the temperature of a liquid is given by  Q = mCΔT where Q =…

Q: How much heat is released when 10.0 g of Steam (water vapor) at 110.0 C is cooled to liquid water at…

A: as  the water vapor is cooled  from 110 degree celcius to 75 degree celcius a heat must be released…

Q: In their Memoir on Heat, published in 1783, Lavoisier andLaplace reported, “The heat necessary to…

A: Given, The specific heat capacity of water is  4.18 J. Initial temperature 0°C. The final…

Q: Calculate the amount of heat required to raise the tempature of an 91 g sample of water from 39C to…

A: Given: Specific heat of water = 4.18 J/g⋅∘C. Mass of water = 91 g. Initial temperature (T1) = 39 ∘C…

Q: Calculate the amount of heat absorbed by 100 g of water that warms from 100 K to 273 K.

A:

Q: How much heat is transferred from a 4.00 g gold nugget (specific heat = 0.129 J/g-°C) initially at…

A: Given : Mass of water = 5 Kg = 5000 g…

Q: How much heat, in joules, would be required to raise the temperature of 450 g of Aluminum (cAl =…

A: Given, mass of Al = 450 g  Specific heat , c = 0.21 cal/g°C  Heat required = ?

Q: Use standard enthalpies of formation to calculate the standard change in enthalpy for the melting of…

A:

Q: A 25.0-g sample of ice at 0.0°C is added to 125 g of water, initially at 35.0°C. What is the final…

A: q1+q2=−q3.... (1), where q1 - the heat absorbed by the solid at  0∘C q2 - the heat absorbed by the…

Q: How much heat will be absorbed by a 59.9 g piece of aluminum (specific heat = 0.930 J/g･°C) as it…

A:

Q: How many kilojoules of heat energy are absorbed by a 200. g block of ice from -10 C to 0 C?

A: Solution-  Given Temperature-  00C to - 100C heat energy are absorbed by block of ice =200. g…

Q: How much heat will be absorbed by a 42.3 g piece of aluminum (specific heat = 0.930 J/g･°C) as it…

A:

Q: How much heat is required to convert 58.2 g of liquid water at 15 °C to water vapor at 125 °C. (Use…

A: Heat absorbed or evolved by any substance depends on it's mass , specific heat and change in…

Q: How much heat (in kJ) will be absorbed by a 75.9 g piece of aluminum (specific heat = 0.930 J/g･°C)…

A:

Q: Sodium chloride, the table salt (NaCl) is added in cooking to enhance the flavor of the food. When…

A: Mass of NaCl = 10 g  Volume of water = 200.0 mL * coffee-cup calorimeter initial temperature = Ti =…

Q: How much heat will be absorbed by a 50.3 g piece of aluminum (specific heat = 0.930 J/g•°C) as it…

A: Mass of Aluminum = 50.3 g Specific mass = 0.930 J/g◦C

Q: How much energy is evolved as heat when 4.7 L of water at 0 °C solidifies to ice? (The heat of…

A: We know that  Density of water = 1 g/mL Mass of water = density of water x volume Mass of water = 1…

Q: 6. Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C.…

A: Given: The mass of ice = 1.0×102 g The amount of heat absorbed by ice = 1255 J The final temperature…

Q: In joules, how much heat is released when 36.0 g of Ag cools from 181. to 129.?

A:

Q: How hot does a thanksgiving dinner roll need to be to warm up and melt a 4.0 g 'pat' of butter?…

A: The heat lost by the rolls is equal to that gained by butter.

Q: Calculate the heat change in kilojoules for freezing 30.0 g of water at 0 ∘C.

A: Heat change in freezing is equal and opposite of heat change in melting or heat of fusion (dHfus).…

Q: How much heat energy is needed to raise the temperature of 10.00 grams of solid aluminum (c = 0.90…

A: Heat energy can be calculated as: Q = mc∆T Where, Q = heat m = mass c = Specific heat ∆T = Change in…

Q: A 20 g sample of ice at -10 °C is mixed with 100 g water at 80 °C. Calculate the final temperature…

A: Heat required by ice to convert into water at 0 oC = ms(Tf-Ti) + mLf…

Q: Using the specific heat data indicated for each question to calculate the amount of heat (in…

A: Specific heat “S” of a substance is generally defined as that heat amount which is needed to…

Q: How

A: We will calculate heat used in conversion of ice into 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.