Calculate the amount of heat needed to convert 230.0 g of ice at -10ºC to water at 0ºC.

Q: snip

A: Formula used: The heat can be calculated as, The change in temperature is calculated as,

Q: Calculate the amount of ice in grams that, upon melting (at 0  C), absorbs 237 kJ of heat.

A:

Q: calculate total amount of heat needed to change 750g of ice at -10C into 750g of water at 84C

A: In order to calculate the amount of heat needed to change the given sample of ice to water of the…

Q: How much heat is absorbed when 10.0 grams of ice initially at -30.0ºC is heated and completely melts…

A: Since in the above process, two steps are happening 1) heating of ice from -30.0 ºC to 0 ºC  2)…

Q: What is the total amount of heat required to convert 35.0 g of ice at -22.9 ºC to water at 40.0 ºC?…

A: Mass of ice = M = 35 gInitial Temperature of ice = Ti = -22.9°CFinal temperature of Ice = T = 40…

Q: How much energy in kJ would it take to heat up 34.823 g of water at 47.8 degrees C until it…

A: Mass of water = 34.823 gm  Moles of water = 34.823/18 = 1.94 moles  Initial temperature = 47.8°C…

Q: How much heat is needed to melt 75.0 g of ice that is at -28.0ºC?

A: We have given that Mass of ice = m =75 grams T1 = -28°C T2 = 0°C ∆T = T2  - T1 = 0  -  (-28) = 28°C…

Q: 1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to…

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Q: How much heat in kilojoules is required to warm 10.0g of ice, initially at -10°C, to steam at 110°C?…

A: Given that: mass of ice = 10 g initial temperature = -10°C final temperature = 110°C Specific heat…

Q: What amount of heat is required to convert a 1.5 kg block of ice at -15.0°C to steam at 150.0°C?…

A: Given, mass of block of ice = 1.5 kg =1500 g

Q: Heat is added to ice at 0°C. Explain why the temperature of the ice does not change. What does…

A: Given : Heat is added to ice at 0 °C.

Q: How much heat (in kilojoules) is evolved in converting 1.00 mol of steam at 130.0 °C to ice at -45.0…

A: Moles of steam  = 1 mol,

Q: How much heat is evolved in converting 1.00 mol of steam at 135.0 ∘C to ice at -55.0 ∘C? The heat…

A: To determine evolved heat:The formula to calculate heat for cooling three phases where it changes…

Q: What amount of heat is required to convert a 1.5 kg block of ice at -15.0°C to steam at 150.0°C?…

A: To solve this problem we will use the formula   q = m•c•∆T  Where,  q = heat requires  m = mass of…

Q: How much heat is needed to raise 63.0 g of ice from  – 10  oC to water at 50 oC at 1 atm?

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Q: Calculate the amount. of heat required to completely evaporate 625 ml of water at 25C. the enthalpy…

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Q: If 8000 cal is needed to change the temperature of a certain amount of ice at -25°C to steam at…

A: Specific heat  of the substance of the  heat capacity of a sample of substance is divided by mass of…

Q: calculate total amount of heat needed to change 500.0g of ice at -10C into 500.0g of steam at 120.0C

A: We have to give 3 energy for this conversion First raise the Temperature from-10°C to  0°C . Then…

Q: What represents the amount of heat released at the condensing point to condense 1 mol of vapor? O…

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Q: How much heat is evolved in converting 1.00 molmol of steam at 135.0 oC to ice at -45.0 oC? The heat…

A: Number of mol of water = 1molSo, amount of water = 18 gInitial temperature, Ti = 135 oCFinal…

Q: 8. How many calories must be removed to change 75g of steam at 200°C to ice at O'C (Sp. Ht. of ice =…

A:

Q: Given the information below, sketch the phase diagram of Nitrogen: Triple point: 0.1252 atm, -210°C…

A: The diagram which shows the physical change of substance at a particular temperature and pressure is…

Q: The vapor pressure of water at 27°C is 25 torr, and the heat of vaporization of water at 27°C is…

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Q: How much heat (in kJ) is evolved in converting 1.00 mol of steam at 145 °C to ice at -50 °C? The…

A: Heat released during the conversion from 145oC to 100oC.

Q: How much energy is required to melt 135 grams of frozen ethanol? Ethanol heat of vaporization is…

A:

Q: How much heat is needed to melt 466 g of silver that is at 22.3 ºC?

A: Given that : Mass of Silver = 466g Initial temperature (T1) = 22.3°C Melting point of Silver (T2) =…

Q: Calculate the amount of heat required to convert 200.0 grams of ice at -40.0°F to steam at 226°F

A: the amount of heat released can be found out by taking the product of mass of substance and change…

Q: How many Joules of energy are required to melt 1.5 moles of ice at 0 degrees celcius?

A: given: moles of ice = 1.5 moles molar mass of ice = molar mass of water = 18 g/mol mass of ice =…

Q: How much energy is required to convert 35.0 g of water at 27.5°C to steam at 155.0°C? (specific heat…

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Q: How much energy (in kJ) is needed to convert 50.0 g of ice at -10.0 ºC to liquid water at 0.0 ºC?

A: M=50 gm=0.05kg  we raise the temperature of 0.05kg of ice at -10C to 0C. The heat capacity of ice,…

Q: At a pressure of 1 atm, kJ of heat are needed to vaporize a 38.7 g sample of liquid benzene at its…

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Q: From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at −4.00…

A: The heat required to change the temperature of 30 g ice from -4.00 to 0.00 oC (q1) is determined as…

Q: How much heat is needed to melt 2.5 grams of ice given that water has a heat of fusion of 6.0…

A: Sine we know that  Heat needed to melt ice = number of mole of ice × heat of fusion  So we will find…

Q: What accounts for the differences in boiling points and heat of vaporization

A: Boiling point and heat of vapourization depends on the the intermolecular forces. Stronger is the…

Q: How much heat must be added to a 2-kg block of ice at -5°C to change it to water at 10°C? C of ice =…

A: Specific heat capacity of water: 4.184 J/(g oC) Specific heat capacity of ice: 2100 J/(kg oC) Latent…

Q: What amount of heat is required to convert a 1.5 kg block of ice at -15.0°C to steam at 150.0°C?…

A: Given the mass of ice block, m = 1.5 Kg = 1.5 Kg * 1000 g1 Kg= 1500 g The required constant values…

Q: How much heat is needed to melt 75.0 g of ice that is at -33 ºC?

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Q: Calculate the amount of heat needed to convert 35.05 g of liquid water at 100°C to a gas. The molar…

A:

Q: What quantity of heat (in kJ) would be required to convert 12.9 g of ice to water at 0.00°C? (∆Hfus…

A:

Q: The enthalpy of fusion of ice (AHfus) is 6.0 kJ/mol at 0 °C. This means kilo joules of heat energy…

A: Given that enthalpy of fusion of ice at 0⁰C is 6.0 kJ/mol. The molar enthalpy of fusion actually…

Q: A total of 537 cal of heat is added to 5.00 g of ice at -20.0 °C. What is the final temperature of…

A: Given data :  Mass of ice = 5.00 g  Initital temperature of ice = -20.0°C Total heat added = 537 cal…

Q: The heat of fusion for ice is 333.6 joules per gram. Adding 333.6 joules of heat to 1.0 gram of ice…

A: The heat of fusion(∆Hf) is the amount of heat energy required to change from solid state to liquid…

Q: Calculate the energy in the form of heat (in kJ) required to change 76.9 g of liquid water at 25.2…

A: Given:  mass = 76.9 g Heat of fustion = 333 kJ heat capacity of water = 4.184 J/g°C heat capacity of…

Q: 1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to…

A:

Q: The heat capacity of liquid water is 4.18 J/g-°C and the heat of vaporization is 40.7 kJ/mol. How…

A: Given data,  Heat capacity of liquid water (s) = 4.18 J/g.°C  Heat of Vaporization(∆Hvap) = 40.7…

Q: Calculate the total energy, in kilojoules, that is needed to turn a 12 g bloc of ice at -40 degrees…

A: Answer:- This question is answered by using the simple concept of heat energy required to convert…

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.