A 466 g of water is heated from 8.50C to 74.60C. Calculate the amount of heat absorbed (in kilojoules) by water. *

Q: How much water is present if 64.9 kJ is needed to heat up water at 17.3°C to 96°C to brew some…

A: The amount of heat transferred from a system is calculated as follows,…

Q: How much heat must be absorbed by a 15.0-g sample of water to raise its temperature from 25.0 °C to…

A: The heat absorbed by the given system is determined by using following formula.

Q: How much heat would need to be removed to cool 50.3 g of water from 25.6°C to -10.7°C?

A:

Q: Calculate how much heat 32.0 g of water absorbs when it is heated from 25.0°C to 80.0°C. Specific…

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Q: A piece of silver releases 202.8 J of heat while cooling 65°C. Calculate the mass of the sample if…

A: Given that, a piece of silver releases 202.8 J of heat while cooling 65 oC temperature. The specific…

Q: Assuming that Coca-Cola has the same specific heat as water [4.18 J/(g⋅∘C)J/(g⋅∘C)], calculate the…

A: given, specific heat (c) = 4.18 J/(gm.°C) mass of the substance(m) = 350 gm initial temperature=…

Q: when hydrogen and oxygen are burned to produce water. heat is produced at 58 kcal mol of water. A…

A: We are given with the heat produced for 6.02×10-23 molecules = 58 KCal. So , to find heat produced…

Q: How much heat in kJ is needed to raise the temperature of 130.0 g of water from 15 degrees Celsius…

A: Given, amount of water =130.0 ginitial temperature Ti =15 °Cfinal temperature Tf =100 °C ( boiling…

Q: A 466 g sample of water is heated from 8.50 degrees C to 74.60 degrees C.  Calculate the amount of…

A: Interpretation-  To determine the amount of heat absorbed (in kilojoules ) when 466 g sample of…

Q: Calculate the amount of heat required to raise the temperatureof a 65-g sample of water from 32oC to…

A: The heat Q required to raise the temperature is,

Q: The specific heat of water is 4.184 J gc. What is the amount of heat associated with heating 50.0 ml…

A:

Q: If 14.5 kJ of heat were added to 485 g of liquid water, what would be the increase in temperature?…

A: Concept introduction- Specific heat- It is the amount of heat required to raise the temperature of…

Q: 1. Relating Heat, Temperature Change, and Heat Capacity a. Large beds of rocks are used in some…

A: Given  (a)     Mass of Rocks ( m ) = 50 kg                                           = 50 × 103 gram…

Q: How much heat is released when 30 g of water at 96°C cools to 25°C? The specific heat of water is…

A:

Q: Calculate the amount of heat absorbed by 23.0 g of water when its temperature is raised from 31.0°C…

A: Answer

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: How much heat is absorbed by a 1.50-g water sample if it is heated from 25.0°C to 38.0°C? The…

A:

Q: During a strenuous workout, an athlete generates 2210 kJ of heat energy. What mass of water would…

A: Q = nΔHvap   where Q is the heat dissipated by the systemn is moles of the compoundΔHvap is the heat…

Q: What mass of water can be heated from 10.0 °C to 75.0 °C using 95.1 kJ of heat?

A:

Q: How much heat is absorbed in kJ by 750 grams of water as it is heated from 25oC to 96oC? Specific…

A: Given- mass of the water= 750 grams  heated from 25oC to 96oC Specific heat of water= 4.186 J/goC

Q: Why does water have a high specific heat index? It requires a great amount of energy for water to…

A: Ans As we all know the water can form strong hydrogen bonding  Hence, Water has a the higher…

Q: 1. Compare the change in temperature values for your data of water compared to the metal in part A.…

A: As per bartleby guidelines, I am allowed to answer one question at a time. Please reupload the rest.…

Q: How much heat is released when 60.5 grams of water at 60.0 degrees C changes to water at 12.5…

A: The question is about calculating the amount of heat released when 60.5 grams of Water at 60oC…

Q: Section 7: Heat 1. When ice melts, describe what happens to the energy of the air around it. 2.…

A: Heat absorption depends on heat capacity of substance.

Q: Determine the amount of heat energy in joules required to raise the temperature of 7.40g of water…

A: Given:  Mass of water = 7.40 g  Initial temperature = 29°C Final temperature = 46°C Standard data:…

Q: If 10 g of water at 52oC and 25 g of water at 10oC were mixed in an insulated container, what will…

A: Given: Specific heat of water = 4.184 J/g°C

Q: How many joules of energy would be required to raise the temperature of 3.2 grams of mercury  4.2ºC?…

A:

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: Given that a 10.0 g sample of ice melts and then the resultant water proceeds to warm to 20.0 C,…

A: Given mass of ice = 10g Process 1: conversion of ice at 0 degree tp water at 0 degree The total heat…

Q: Assuming that Coca-Cola has the same specific heat as water [4.18 J/(g C)], calculate the amount of…

A: Given: Mass = 350g Temperature (initial) =  300C Final temperature = 90 C

Q: The specific heat of mercury is 0.140 J/g°C. Calculate the heat necessary to raise the temperature…

A:

Q: How much heat is liberated when 50g of water is cooled from 100 ᵒ C to 20 ᵒ C

A: This can be solved as follows

Q: How much heat is put into 100g of water to raise temperature from 25.0 to 75.0°C? The specific heat…

A:

Q: How much heat would need to be removed to cool 81.5 g of water from 25.6°C to -10.7°C?

A: Given that:  Mass of water (m) = 81.5 g  Initial temperature (T1) = 25.6°C Final temperature (T2) =…

Q: How many kilojoules of heat are absorbed when 2.00 L of water is heated from 12.5°C to 93.5°C?

A: Mass= density×volume  Mass= 1×0.002=0.002gm Now  Q=mc∆T Q= 0.002×4.18×(93.5-12.5) Q= 0.067×10-6kj

Q: If 40.0 kJ of energy is absorbed by 500.0 g of water at 10.0 oC, then what is final temperature of…

A: Q = m . s . (T2-T1)

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: Because water has such a high specific heat capacity, it heats and cools more slowly than land. How…

A: Given that,

Q: A hot pot of water is set on the counter to cool. After a few minutes it has lost 335 J of heat…

A: In this question, we will determine the heat energy gained by the surrounding.  You can see the…

Q: How much heat is required to warm 100.0 g water from 31.8 degrees Celcius to 67.5 degrees Celcius?…

A: The heat required is calculated as,

Q: How much heat (in kilojoules) is gained by 294 grams of water that is warmed from 25.00C to 57.00C?…

A:

Q: The specific heat of water is 4.184J/g-°C. How many joules of heat will be  removed from 2.00 g of…

A: Given: Decrease in the temperature of water = 20.0 oC And mass of water = 2.00 g

Q: Relate the heat gained by the calorimeter and water with the heat lost by the metal. EXPLAIN

A: The heat gained by the calorimeter or water is always equal to the heat lost by the metal.This the…

Q: Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC?…

A:

Q: For copper, with a Hfus of 209 J/g, how many kilojoules of energy will be absorbed or released when…

A:

Q: The specific heat capacity of silver is 0.2386 J/g °C. Assuming no loss of heat to the surroundings…

A: The specific heat capacity of silver is = 0.2386 J/goC The mass of silver is = 100.0 g The initial…

Q: How much energy must be absorbed by 20.0 g of water to increase its temperature from 283.0 °C to…

A: The answer is given as follows

Q: The specific heat capacity of liquid mercury is 0.14 J/g-K. How many kilojoules of heat are needed…

A:

Q: If 57600 J of energy were absorbed by 250. g of water at 0.0 ̊C, what would be the final…

A:

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.