A particular refrigerant cools by evaporating liquefied CCI 2F 2. How many kg of the liquid must be evaporated to freeze a tray of water to ice (at zero degrees C)? The tray contains 525 grams water. Molar heat of fusion of ice = 6.01 kJ/mol. Molar heat of vaporization of CCI 2F 2 = 17.4 kJ/mole 87.2 kg 6.02 x 10 1 kg 1.22 kg 5.20 x 10-2 kg 169 kg 36.8 kg 71.3 kg 0.504 kg O O OO O O O C

Q: What mass of molybdenum (molar mass=95.94g/mol) is needed for the mercury to release 600.0J of…

A:

Q: 13. A sample of ice at 0°C melts after absorbing 300,000J of heat. How many moles of H,0 are…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: A 125.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A: Concept - In the question, because the substance is getting cooled, there will be release in the…

Q: 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice,…

A: Moles of Na = mass/molar mass = 0.250g/(22.99gmol-1) = 0.01087 mol 2 moles of Na produces 368 kJ of…

Q: A 0.790-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at…

A: The relation of heat energy, mass, heat capacity and change in temperature can be given as…

Q: Suppose that 1.15 g of rubbing alcohol (propan-2-ol) evaporates from a 65.0 g aluminum block. If…

A: Given, Mass of alcohol evaporate = 1.15 g Mass of Aluminum block = 65.0 g Initial heat of the block…

Q: A 17.5-g sample of ice at –11.6°C is mixed with 119.8 g of water at 80.0°C. Calculate the final…

A: The phase change involving different substances always occur after gaining/losing a specified heat.…

Q: A 22.5-g sample of ice at 0.0 oC is added to 100.0 g of warm water at 35.0 oC, and the final…

A: Given : Mass of ice = 22.5 g Initial temperature of ice = 0.0 oC Final temperature of mixture =14.0…

Q: The following information is given for silicon at 1 atm: = 2355.00°C   (2355.00°C) = J/g =…

A:

Q: A 417.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C.…

A:

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

A: The heat required to boil off water is calculated as shown below: Heat = Heat required to raise the…

Q: Suppose that 1.01 g of rubbing alcohol (C3H8O) evaporates from a 65.0 g aluminum block. Aluminum has…

A: Given data:

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

A:

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

A:

Q: The following information is given for tin at latm: boiling point = 2270 °C AH-ap(2270 °C) = 230…

A: The mass of liquid tin is = 22.4 g The temperature of the liquid tin is = 232oC The heat of fusion…

Q: Based on the thermodynamic properties provided for water, determine the energy change when the…

A:

Q: Ethyl chloride, C2H5CI, is used as a local anesthetic. It works by cooling tissue as it vaporizes.…

A: The molar mass of ethyl chloride is : MC2H5Cl=M2C+M5H+MCl           =[12×2+5×1+35.5]           =64.5…

Q: Two 20.0 g ice cubes at -14.0 °C are placed into 265 g of water at 25.0 °C. Assuming no energy is…

A: Answer: This question is based on the principle of conservation of energy which suggests that heat…

Q: A 123.6 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 is 123.6 g. Molecular mass is 189.50 g/mol. Heat capacity of liquid is 1.62…

Q: How many joules of energy are required to change 50.0 g of Cu from 25.0°C to a liquid at its melting…

A: Given:  Mass of Cu given= 50.0 g  Initial temperature= 25°C  Final temperature= 1083°C  Specific…

Q: Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is…

A: Given  System is isolated that means Heat is not transferred from the system on surrounding . When…

Q: Calculate the amount of energy that is released when 400 grams of water vapor cools from 115oC to…

A: To solve this problem we have calculate energy released during temperature change and phase change…

Q: 22) Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the…

A: Two questions based on chemical thermodynamics, which are to be accomplished.

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: Determine the heat in joules to melt 52.75 moles of water given the heat of fusion is 6010 J/mol?

A: Heat of fusion is the amount of energy required for melting a given mass at its melting point…

Q: A 417.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C.…

A: To solve this problem we will use the formula  q = m•c•∆T  Where, q = heat absorbed or released  m =…

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

A:

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

A:

Q: Two 20.0‑g ice cubes at −20.0 ∘C are placed into285 g of water at 25.0 ∘C. Assuming no heat is…

A: Given information: Mass of ice = 20.0 g Mass of water = 285 g Initial temperature = -20 ℃ Final…

Q: Two 20.0 g ice cubes at −16.0 ∘C−16.0 ∘C are placed into 255 g255 g of water at 25.0 ∘C.25.0 ∘C.…

A: Given data:

Q: Ice at -4.80oC is added to 220g of water at 26.60oC. What is the mass of ice needed to cool the…

A: Mass of water = Mw = 220 gMass of ice = to be determined Initial Temperature of water = Tw =…

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: A 125.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A:

Q: A 389.7 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C.…

A: Mass of unknown sample = M= 389.7 gMolar Mass of Unknown Sample = 92.41 g/moleNo of moles of Unknown…

Q: how much energy is required to vaporize 48.7 g of dichloromethane at its boiling point. (31.6…

A: We need to find the energy required to vaporize.  Mass = 48.7 g Boiling point = 31.6 kJ/mol

Q: The enthalpy for boiling water is 40.7 kJ/mol. How much heat is required to boil 250.1 g of water?

A: Number of moles of any substance can be calculated by dividing the mass withits molar mass which may…

Q: If 100.0 g of ice at -10.0°C is placed in 200. g of water at 90.0°C in an insulated container, what…

A: Given : Mass of ice = 100.0 g Initial temperature of ice = -10.0 oC Mass of hot water = 200 g And…

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

A:

Q: 8. The heat of vaporization of benzene (C2H6) is 568 J/g. How much energy is needed to vaporize 4.5…

A: Chemical formula of benzene is C6H6. Mass of 4.5 moles of benzene = moles x molar mass = 4.5 x 78 =…

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: A 110.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C.…

A: Mass of the unknown substance= 110.1 g Heat capacity of liquid = 1.62 J/g･°C Heat capacity of the…

Q: Two 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is…

A: Quantity of heat absorbed =  Quantity of heat emitted Heat required for melting = moles of substance…

Q: Calculate the mass of ice required to cool 181 mL of beverage from 24.6 °C to 0.0 °C. Assume a…

A: First find the heat lost (q) by the beverage. Then using the obtained “q” value and given enthalpy…

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: Given that a 10.0g sample of ice at 0.0 degrees celsius melts and then the resultant water proceeds…

A: Note: As per our code, we are allowed to answer only the first question when a collection of…

Q: Two 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is…

A:

Q: A 0.870-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at…

A: The moles of Li can be calculated as, mass of lithium, Li = 0.870 g Molar mass of Li= 6.941 g/mol…

Q: Lead has a melting point of 327 °C, its specific heat capacity is 0.13 J/g °C and its molar enthalpy…

A: The given problem can be solved by the following calculations as; Heating lead from 20.4°C  to…

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…

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.