A 450 g H2O is heated from 11.5oC to 81.0oC. Calculate the amount of heat absorbed (in kilojoules) by H2O.  Specific heat of H2O: 4.184 J/g oC

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

A:

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

A:

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: Use the information provided to calculate the quantity of heat (in kJ) required to convert 73.4675 g…

A: the question is based on the concept of Hess law. according to Hess law,  net enthalpy change for…

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: what is the relation of heat gained by the ethanol to the heat lost by the metal

A: When ethanol comes in contact with the  metal which has higher temperature than ethanol then the…

Q: 1. How many grams of a metal with a specific heat of 0.103 J/gC when transferred from boiling water…

A: At equilibrium,  Heat lost by the metal = Heat gained by water

Q: A calorimeter of mass 125 g contains 130 g of water at 20 ᵒC. A 6.1-g mass of steam at 100 ᵒC is…

A: Given : Mass of calorimeter = 125 g Mass of cold water = 130 g Initial temperature of cold water and…

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: 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: 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: Which of the following statements is true? Specific heat capacity is dependent on the amount of the…

A:

Q: Which substance has zero Gibbs free energy of formation?  A. N2 (g) B. CO2 (g) C. MgO (s) D.…

A: When an element is presebt in its native or standard state, its gibbs free energy of formation will…

Q: Calculate the heat released when 1.735 L O2 with a density of 1.11 g/L at 25°C reacts with an excess…

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: Ethanol, CHsOH, boils at 78.29 C. How much heat energy (in kilojoules) is required to heat 1.40 kg…

A: Total heat required for this phase change is the sum of change during these two process 1. Change…

Q: If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?…

A:

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

A:

Q: Given that the reaction of ozone forming oxygen below has a heat of reaction of – 286 kJ…

A:

Q: 23.  Calculate the mass of water in grams that can be heated from 0 oC to 15 oC by the amount of…

A: Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg…

Q: How much heat (in kilojoules) is gained by 231 grams of water that is warmed from 25.00C to 39.00C?…

A: Given: Mass of water=231 g Temperature change, ∆T=(39.0-25.0)°C=14 °C The heat gained q =? kJ…

Q: How much heat was absorbed (in J) if a 19.6 g sample of an alloy with a specific heat of 0.316 J/g…

A:

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: 236 grams of water at 11°C is subjected to a big fire. Calculate the heat in kJ, absorbed by H20…

A: Given that: mass of water = 236 g T1 = 11 oC T2 = 173 oC ∆Hvap = 2260 J g-1 Specific heat of water…

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: 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: If 15.5 J of heat are removed from 14.6 g of mercury (specific heat = 0.142 J/g oC) at 25.0 oC, what…

A: From the formula of specific heat capacity we can determine the final temerature of mercury sample .

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

A:

Q: Ethanol, CHsOH, boils at 78.29°C. How much heat energy (in kilojoules) is required to heat 1.40 kg…

A: A numerical problem based on heat energy released, which is to be accomplished.

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: 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 heat change, in kilojoules, when 72.3 g of water in the form of steam are cooled from…

A: The mass of water is 72.3g.Molar mass of water is 18.01528g/mol.

Q: Calculate the total enthalpy change (kJ) for the following reaction:   H2O (s, 90 g, –10. oC)…

A: In the above process, 3 steps are involved 1) Heating of 90 grams ice from –10 oC to 0 oC  2) fusion…

Q: How many moles of H2 are required to give off 2551 kJ of heat in the following reaction? N2 (g) + 3…

A: Heat of Rxn = -91.8 KJ/mol Q = 2551 KJ

Q: How much heat(in kJ) is absorbed when 75.0g of benzene at -15°C is cooled to 35°C? mp = 5.85°C,…

A:

Q: Part A)   The standard molar heat of formation of water vapor (steam) is -242 kJ/mol. What amount…

A: Only first question is answered according to the policy

Q: If it takes 41.0 kJ of heat to melt 200.0 g of copper, calculate the AHfus in kJ/m

A: The number of moles of a substance is given as the mass of the substance upon its molar mass. 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: How much heat must be absorbed by 375 grams of water to raise its temperature by 25° C? Specific…

A: Given, mass = 375 g  Specific heat, c = 4.184 J/g°C  Heat = ?

Q: Given that the reaction of ozone forming oxygen below has a heat of reaction of – 286 kJ…

A: Enthalpy change:The amount of energy lost or acquired during a reaction is approximately…

Q: A 466 g of water is heated from 8.50C to 74.60C. Calculate the amount of heat absorbed (in…

A: Given,  Mass of water = 466 g  Heat absorbed = ?

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

A:

Q: How much heat is absorbed by a 275-gram sample of water as it is heated from 25oC to its boiling…

A: The heat absorbed by a substance is dependent upon the nature of the material (specific heat…

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates). 

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.