What quantity of heat (in J) would be required to convert 6.91 mol of a pure substance from a liquid at 40.0 °C to a gas at 113.0 °C? + Cliquid = 1.45 J/mol °C Tboiling = 88.5 °C Cgas = 0.65 J/mol•°C AHvaporization = 1.23 kJ/mol

Q: What quantity of energy, in joules, is required to raise the temperature of 455 g of tin from room…

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Q: A 153.7 g sample of ice at 0.0 °C is added to 150.7 mL of liquid water at 67.8 °C in a styrofoam cup…

A: All the required calculations have been done in the following step.

Q: If 46.1 g Zn (Cp=0.388 J/g°C) at 18.0 °C is placed in 80.0 g of water at 75.0 °C (Cp = 1.00…

A:

Q: The specific heat of gold is 0.129 J/g.oC. What is the molar heat capacity of gold (Au)? 0.129…

A: Since the relationship between the specific heat capacity and molar heat capacity is  Molar heat…

Q: Benzene (C6H6) is an organic compound that boils at 80.1°C. If 100.0 grams of liquid benzene at…

A: The heat of Vapourisation is the amount of energy that must be added to the liquid substance to…

Q: How much energy is required to heat 100.0 g acetone (molar mass=58.08 g/mol) from a solid at…

A: In this question, we want to determine the amount of energy is required to heat 100.0g acetone from…

Q: Substance D has the following properties: ΔHvap = 30.5 kJ/mol ΔHfus = 5.9 kJ/mol Tb = 89.4 °C Tm…

A: Mass of substance =107.6 grams Molar mass of substance =75 grams Numbe rof moles of substance=Mass…

Q: 4) The table below contains thermodynamic values for water (H20) and for methane (CHA). Water…

A: The enthalpy of fusion (∆Hf) is termed as the quantity of energy that must be supplied to convert…

Q: The temperature of 13.48 g of C2H6O increased by 9.08°C when heated. How much heat did it absorb if…

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Q: How much heat (in J) would be required to convert 2.31 mol of a pure substance from a liquid at…

A: Given: Moles of substance = 2.31 mol. Initial temperature of substance = 40.0 oC And final…

Q: A 500 g piece of iron (CP = 25.09 J/(mol · °C) changes 7°C when heat is added.  How much heat energy…

A: Given mass of iron = 500 g Molar mass of iron = 55.85 g/mol Number of moles of iron = 500/55.85 =…

Q: Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C&H6) from 0.00 °C to…

A: Given that: molar mass: 78.11 g/mol cs,solid  = 1.51 J/g*°C cs,liquid  = 1.70 J/g*°C cs,gas  = 1.05…

Q: If 40.0 g of hot water at 80.0oC is added to 60.0 g of cold water at 20.0oC, what is the final…

A: The final temperature is 44 oC

Q: At a certain elavation, the boiling point of water is 98.5C. How much energy, in kilojoules, is…

A: Heat energy needed,Q= 11.0 KJ

Q: sample of water weighing 46 g is heated from 8.5 Cº to 74.6 C°. Calculate the amount of heat…

A: Given data: Mass of sample of water = 46g Water specific heat =  4.184 J/g C° Initial temperature =…

Q: How much heat, in joules, must be added to a 75.0 g block of a metal alloy with a specific heat of…

A: Given, Mass of the substance, m = 75.0 g Initial temperature, T1 = 25 oC Final temperature, T2 = 775…

Q: How much heat is required to vaporize 100.0 g of ethanol

A: Number of moles = mass ÷ molar mass  Molar mass of ethanol is 46.07 g/mol

Q: nge. Given the following information for ethanol, C2H3OH (at 1 atm), calculate the amount of heat in…

A: The correct answer is given below

Q: If 29.00 g of aluminum at 76.45 °C is dropped into 125.7 g of water at 34.04 °C, what will be the…

A:

Q: energy

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Q: 54.73 g of water, H2O, 18.02 g/mol, was heated from -19.53 °C to 112.08 °C.  The freezing and…

A: Between the heating range of -19.53 to 112.08 degree all three states of water is present. At -19.53…

Q: What quantity of heat (in kJ) is evolved when 25.0 g H2O(g) at 125.0 °C is converted to H2O(l) at…

A: we have to calculate the heat evolved when 25.0 g H2O(g) at 125.0 °C is converted to H2O(l) at 35.0…

Q: A substance, X, has the following properties. (Size of mass is 250. g.) Specific Heat Capacities…

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Q: Calculate the quantity of energy required to convert 72.8 g of H₂O(s) at 0.0 °C to H₂O(g) at 100.0…

A:

Q: Water exists as a liquid at room temperature (25.0°C). If 300 kJ of heat energy is added to 100 g…

A: Answer:Increasing the temperature of liquid water up to its boiling pointVaporization of…

Q: Suppose that 1.07 g of rubbing alcohol CH₂O evaporates from a 750 g aluminum block Aluminum has a…

A: Answer:When rubbing alcohol will be evaporated then it will gain heat in that process and that heat…

Q: 11. 100.g of Cu at 100°C is added to 150.g of H2O at 10.0°C. If the specific heat of copper is 0.389…

A: The amount of energy going out of the warm water is equal to the amount of energy of the cool water.

Q: Calculate the mass of liquid water (in grams) at 100 °C that can be converted to vapor when 2400 J…

A: Calculate the number of moles of liquid water which can be converted into vapor form on absorption…

Q: heat of vaporization (kJ/mol) of methanol.

A:

Q: How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C…

A: Acetone first raises its temperature from -154°C to its melting point, then the solid acetone melts…

Q: Energy Constants for H2O 334 J/g = Heat of Fusion (Hf) 2260 J/g = Heat of Vaporization (Hv) 2.11…

A: Answer:- This question is answer by using the simple concept of calorimetry which state that heat…

Q: 7. An old "trick" for cooling down a hot beverage quickly is to immerse a cold spoon into the…

A: Since the hot coffee is at a higher temperature, it releases heat and the silver spoon accepts heat…

Q: Liquid ammonia (boiling point = –33.4°C) can be used as a refrigerant and heat transfer fluid. How…

A: Liquid ammonia (boiling point = –33.4°C) can be used as a refrigerant and heat transfer fluid. The…

Q: Ethanol, C₂H5OH, boils at 78.29 °C. How much energy, in joules, is required to raise the temperature…

A: Given, Note: 1 kg = 1000 g mass of ethanol = 3.00 kg = 3000 g Initial temperature (Ti) = 43.0 °C…

Q: The specific heat capacity of water is _____.     (g x °C)/1 cal °C/(g x 1 cal) 1 cal/(g x °C) g/(1…

A: The specific heat capacity denoted by Cp is the amount of energy that must be supplied to 1 unit…

Q: Ethanol, C2H5OH, boils at 78.29°C. How much energy, in joules, is required to raise the temperature…

A:

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: Calculate the heat in kJ for 175 g of water vapor condensing to liquid water from 228.0 oC to 175.0…

A: Given: Mass of water vapour = 175 g Initial temperature (T1) = 228°C Final temperature (T2) = 175°C…