How much heat is required to boil 62.0 g of water at its boiling point? Express your answer numerically in kilojoules. • View Available Hint(s) ΑΣφ ? kJ

Q: The evaporation of water is endothermic:H2O(l) → H2O( g) ∆Hrxn = +44.01 kJWhat minimum mass of water…

A: Determination of no. of mol of H2O that will evaporate from 175 kJ/mol: n=175 kJ44.01 kJ/mol=3.9764…

Q: If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is ΔHcond for…

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Q: In a freezer, 125 g of water at 0 °C is placed in an ice cube tray. How much heat, in kilojoules,…

A: Given: Mass of water = 125 g.

Q: 3. Recalculate the latent heat of fusion, assuming that 5.0 grams of water were transferred to the…

A: Find the latent heat of fusion, Lf, according to Lf = q÷m by dividing the heat, q, absorbed by the…

Q: Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 23.4 g…

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Q: When 1 mol of CS₂(l) forms from its elements at 1 atm and 25C, 89.7 kJ is absorbed, and it takes…

A: The enthalpy change of the following reaction is ∆H1. The enthalpy change of the following reaction…

Q: A 5.34g sample of aluminum at 23oC absorbs 170 J of heat.  What is the new temperature of the…

A: According to the law of calorimetry Heat absorbed by a substance depends on mass of the substance,…

Q: e net change in enthalpy for

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Q: How many kilojoules of heat energy are going to be absorbed by a pot of water with the mass of 200.…

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

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

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

Q: Given: q = mass X specific heat X (Tfinal - Tinitial) specific heat of water is 4.184 J/g oC How…

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Q: How to calculate the experimental value for the latent heat of fusion of water. 1969.4 cal heat…

A: Latent heat of fusion is the amount of heat required to melt 1 mol or ice at its melting…

Q: Using the equations H2 (g) + F2 (g) → 2 HE (g) AH° = -79.2 kJ/mol C (s) + 2 F2 (g) → CF, (g) AH° =…

A: H2 (g)  +  F2 (g) ----->   2HF (g)  ∆H1° = -79.2 kJ/mol  .................(1) C (s) + 2F2…

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

A: The standard enthalpy of formation of H2O (l) = - 285.8 kJ/mol The standard enthalpy of formation of…

Q: What is the formula to calculate heat energy required to raise the temperature of any substance? O…

A: we need to select the correct formula to calculate heat energy needed to raise the temperature of a…

Q: (a) Consider the following thermochemical data to: 2CO2(g) → 2 C (s, graphite) + 2 O2 (g) AH° =…

A: The enthalpy change of an reaction is extensive property i.e on changing the stoichiometry of…

Q: If a 2.0 g sample of water at 5.0° C absorbs 21.8 of heat energy, what will the temperature of the…

A: given data is  q=21.8, m=2.0g  water heat capacity is 4.18J/g °c apply the formula of heat capacity…

Q: If 1410 J of heat energy is applied to 100g water at 25°C, what will happen? Show using equations to…

A: The amount of energy absorbed or released by a substance is given as; Q = mCdT where Q=energy, m =…

Q: 1.75g CaCl2 dissolves 125g H2O in calorimeter, temp increases 2.44 degrees. what is heat change per…

A: Given that, Amount of CaCl2  w = 1.75 g Molar mass of CaCl2  Mw  = 110.98 g/mol Weight of water in…

Q: A flask of 10 g of diethyl ether is cooled from 50.0 °C to 10.0 °C. What is the total quantity of…

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Q: How much heat does it take to raise 50.0 g of liquid water to 120 °C if its initial temperature is…

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Q: A gold coin whose mass is 8.75 g is heated to 121.1°C and then quickly dropped into an ice…

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Q: Write a balanced thermochemical expression depicting the formation of 1 mol of the compound below…

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Q: Using a coffee-cup calorimeter it was found that when an ice cube weighing 24.60 g melts, it absorbs…

A: ∆H ( enthalpy of fusion ) for this melting process is calculated in kJ/mol using formula :  ∆H = q /…

Q: 1. In what direction does heat flow between two objects? 2. How do endothermic processes differ from…

A: Heat is mode of transfer of energy from one body to another body. There are many other methods to…

Q: The familiar "ether" used as an anaesthetic agent is diethyl ether, C4H20O. Its heat of vaporization…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: What is the resulting temperature when 100 g of water at 75°C is mixed with 30 g of ice at 0 °C?…

A: Mass of water =Mw = 100 g Temperature of water Tw = 75°C Specific heat of water =cw =  4.184 J/g°C…

Q: If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is ∆Hcond for…

A: Given: Heat= 14.8 kJ Mass of HCl= 1.6g To find: ∆Hcond for the substance

Q: How much energy is needed to completely boil away 250 g of 40oC water into 100oC water vapor?

A: Q =q1 + q2  q1 = heat required to warm the temperature  q2 = heat required to vapourize the water…

Q: Calculate the molar heat of formation of solid PCI5 from the following information. P4 (s) +6 Cl2…

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Q: When 1 mol of CS2(l) forms from its elements at 1 atm and 25 ° C,  89.7 kJ  is absorbed, and it…

A: Hess law of constant heat summation: This law states that regardless of the multiple stages or steps…

Q: Based on the thermodynamic properties provided for methanol (below), select from the following list…

A: Given : Mass of methanol = 5.0 Kg = 5000 g Initial temperature of methanol = -64 oC Final…

Q: Calculate the mass of water (H,O, CHO = 4.181 J g-l °C-) at 20.0°C that would be requireć to cool a…

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Q: What amount of heat energy (in Joules) is needed to heat 4.83 grams of water (c = 4.18 J/g°C) at…

A: The given data contains, mass  = 4.83 g. Temperature T1 = 400C Final temperature T2 = 600C

Q: What is the change in temperature (in oC) when a 37 g sample of graphite (specific heat = 0.720 J/(g…

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Q: en the thermochemical equation 2S02(g) + O2(g) – 2SO3(g), AH°rxn-198 kJ/mol, how much heat is evolod…

A: Answer and explanation is given below hope you like it.

Q: Which produces more heat?Os(s) ⟶ 2O2(g) ⟶ OsO4(s)orOs(s) ⟶ 2O2(g) ⟶ OsO4(g)for the phase change…

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Q: Using the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° =…

A: It is given that the enthalpy for the reactions, H2(g) + F2(g) → 2 HF(g) ∆H° = -79.2 kJ/mol  C(s) +…

Q: 76. The evaporation of water is endothermic: H2O(1) – → H,O(g) AHxn = +44.01 kJ %3D What minimum…

A: The evaporation of water is an endothermic process. The enthalpy of evaporation is given by: The…

Q: H2O -286 KJ 2. Prove that the enthalpy change of formation is equal to the total change of enthalpy…

A: Given,  Enthalpy of formation of (ΔHf) of CO2 = -393 KJ  Enthalpy of formation of (ΔHf) of H2O =…

Q: 2. 100 g of water (specific heat = 4.184 J/g. C) and 100 g of a metal sample (specific heat = 0.397…

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Q: How much energy is needed to convert a 55 gram sample of solid potassium at 25°C to liquid potassium…

A: Given thag,  Amount of solid potassium, m= 55 g Temperature of solid potassium Ts = 25°C Temperature…

Q: What is the heat gained by the ice inside the calorimeter if the heat lost by the warm water inside…

A: Calorimeter is an object useful for measuring heat of a chemical reaction.

Q: Which pack had the greatest change in enthalpy? How do you know?

A: Assuming that the material present inside both the packs are of the same specific heat as it is not…

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: How much heat is required to raise the temperature of a 825 g block of wood (specific heat = 1.8 %3D…

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

Q: 30.0 g of a substance (molar mass: 46 g/mol) required 262 J of heat to raise its temperature from…

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Q: What is the mass of a sample of alcohol (specific heat = 2.4 J/g°C), if it requires 4780 J of heat…

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

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…

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.