Suppose you heated a sample of 12.20 grams of water at its boiling point until it completely vaporized. How many kilojoules of heat were used for the vaporization process? Given AHvap = 40.6 kJ/mol

Q: Given that a 10.0 g sample of ice at 0.0 °C melts and then the resultant water proceeds to warm to…

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Q: How about for this one? Benzene, C6H6, boils at 80.1°C. How much energy, in Joules, is required to…

A: Here we have to determine the heat3 energy required to convert 54.68 g benzene ( s) at -30°C to…

Q: How much heat is required to heat a 18.4 g ice cube from -23.0 °C to -1.0 °C? Specific heat of ice…

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Q: Calculate the kilojoules released when 80.0 g of steam condenses at 100 ∘C, the liquid cools to 0…

A: Given : Mass of water = 80.0 g Initial temperature of water = 100 oC = boiling point temperature of…

Q: How much energy is required to vaporize 125 g of benzene, C6H6, at its boiling point, 80.1 °C? (The…

A: The heat of vaporization is the energy required to convert a substance at its boiling point to…

Q: 125 g of dry ice (solid CO2) is dropped into a beaker containing 500 g of 66°C water. The dry ice…

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Q: You mix 18.0g of ice that's at -25.0C with 150.0 mL of water that's at 38.0C. Once the ice has…

A: Heat released is given by  Q = m c (T2-T1) Where m is the mass of the substance  C is the specific…

Q: Calculate the energy absorbed/released, in kJ, when 12.72 g of liquid water is turned to ice. Be…

A: In liquid state water molecules have less intermolecular forces of attraction compare to solid.

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: tion 9 of 10 > The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when…

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Q: 1.82 Benzene (C,H6) is an organic liquid that freezes at 5.5 °C (see Figure 11.15) to form…

A: Given, Temperature = 5.5°C Mass = 15.5 g Enthalpy Change of fusion = 9.95 kJ mol-1

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: 115.4 g of water, H2O, (molar mass is 18.02 g/mol) was heated from -11.54 °C to 135.72 °C. The…

A: The specific heat of a substance is the amount of heat required to raise the temperature of a…

Q: How much energy is needed to cause 5.0x104 g of ice to heat from -40 C to its melting point and then…

A: Matter around us exist in mainly three states, that is solid, liquid and gas. The matters change…

Q: how many moles of water are present if 53.3 kJ of heat are required to melt a sample of ice at 0°C?…

A: • The melting of ice can be represented as,                  H2O(s) → H2O(l)    • The values…

Q: How much energy in kilojoules is required to convert 100mL of water at its boiling point from liquid…

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Q: What change in energy is required to heat 55.00 g of water at 15.00 degrees C to vapor at 180.0…

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Q: A substance has a molar mass of 82.95 g/mol. A 33.5g sample of this substance absorbs 5.114 kJ when…

A: Molar heat of fusion :- The amount of heat absorbed when one mole of a substance changes from solid…

Q: How much heat is absorbed when 25.0g of water warms from 10.2oC to 38.0oC

A: According to calorimetry,  q = m × c × ∆T Where q = heat released or heat absorbed,   c = specific…

Q: Two 20.0 g ice cubes at −21.0 ∘C−21.0 ∘C are placed into 265 g265 g of water at 25.0 ∘C.25.0 ∘C.…

A: The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the…

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: 6.75 When 1 mol of CS,(I) forms from its elements at 1 atm and 25°C, 89.7 kJ of heat is absorbed,…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: The heat of fusion of acetic acid, the principal organic component of vinegar, is 192 J/g. How much…

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Q: w many grams of liquid CF2CI2 are needed to cool 126 g of water from 44.1 to 26.3 °C? The specific…

A: CF2Cl2  chemical name is dichlorodifluoromethane   , it is colourless gas and  it is usually called…

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: Calculate the total energy, in kilojoules, that is needed to turn a 20 g block of ice at 0 degrees C…

A: Total heat required is the sum of heat required in each step.

Q: Two 20.0 g ice cubes at −21.0 ∘C are placed into 215 g of water at 25.0 ∘C. Assuming no energy is…

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

A: To raise the temperature from 28ₒC to 78.29ₒC, required heat is Q1 = m × c × ∆T   = 4000 g × 2.44 J/…

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

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Q: The enthalpy for boiling water is 40.7 kJ/mol. How much heat is required to boil 820.1 g of water?

A: The given question can be solved by calculation the number of moles present in the given amount of…

Q: How much energy is needed to convert 64.0 grams of ice at 0.00°C to water at 75.0°C?  Specific heat…

A: Given, Specific heat (ice)= 2.10J/(g°C) Specific heat (water)=4.18J/(g°C) Heat of fusion= 333J/g…

Q: How much heat energy must be removed from 1.2 g of lead (specific heat = 0.128 J/g ºC) to cool it…

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Q: A 413.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A: Given,mass of sample =413.1 gMolar mass of sample = 189.50  g/molTemperature changed = 233.0°C to…

Q: How much heat (in calories) is absorbed when a 2.60 kg block of ice melts into a liquid? For water,…

A: Given: The mass of ice block, (m) =  2.60 Kg = 2600 g. The ∆Hfus for water=80 cal/g.

Q: Useful Information: Specific heat of water, H2O(t) = 4.18 J/g-"C Specific heat of ice, H;0(s) = 2.04…

A: Note: As per our guidelines, we are supposed to answer only the first question (i.e. question number…

Q: Calculate the energy (in kJ) required to convert 175 g of water from ice at -25.5 °C to liquid water…

A: Given, amount of water =175 gwe are asked to calculate the energy (in kJ) required to convert 175…

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: How much energy does it take to heat 125g of steam from 100 degrees Celsius to 110 degrees Celsius?…

A: Heat in kilojoules can be calculated using the specific heat capacity, temperature difference and…

Q: Benzene has a boiling point of 80.1 °C, and a specific heat capacity of 1.8 J/g °C in the liquid…

A: The heat released in the cooling of any substance in the same phase is given by the following…

Q: How much energy is released when 75.3 g of water vapor at 115 °C condense and cool to liquid at 25.0…

A: Given that : Mass of water (m) = 75.3 g Initial temperature = 115°C Final temperature = 25.0 °C The…

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: 1. How much heat is released when 165 g of liquid benzene, C6H6 (1), cools from 78.0°C to 12.0°C?…

A: The mass of benzene is = 165 g The decrease in the temperature of the liquid benzene is = 78.0oC to…

Q: How much energy is required to vaporize 250 g of water at its boiling point?

A: The energy required for the vaporization of water can be calculated from the standard value of the…

Q: How much heat, in calories, is required to heat a 18.4 g ice cube from -23.0 °C to -1.0 °C? Specific…

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Q: amount of heat released

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Q: Calculate the heat change in calories for condensation of 13.0g of steam at 100 degrees

A: Given : Mass of steam = 13.0  Since condensation is a process in which the steam loses its latent…

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…

Q: How

A: We will calculate heat used in conversion of ice into water

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.