Given the thermodynamic information below for ethylene glycol (molar mass = 62.068 g/mol): Normal melting point: -12.9 °C Normal boiling point: 197.3 °C Enthalpy change of fusion: 9.9 kJ/mol Enthalpy change of vaporization: 65.6 kJ/mol Molar heat capacity for the liquid phase: 149.5 J/mol K Molar heat capacity for the gas phase: 78 J/mol.K Determine the minimum amount of heat needed to vaporize an 18.0-g sample of ethylene glycol initially at 25.0 °C. Consider that all processes occur at 1 atm. Select one: a. h 34.1 kJ 747k1

Q: The fluorocarbon C2Cl3F3 (molar mass: 187.38 g mol-1) has a normal boiling point of 47.6°C. The…

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Q: The normal boiling point of naphthalene, C10H8, is 218 °C. What is the its enthalpy of vaporization…

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Q: Calculate the heat required to completely convert 8.25 g of solid benzene (heat of fusion 9.92…

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Q: Two 20.0 g ice cubes at -20.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is…

A: In the given question we have to calculate the final temperature in the given conditions.The heat of…

Q: a) What is the heat of vaporization of carbon tetrachloride, in kJ?

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Q: What amount of ethylene glycol (molar enthalpy of vaporization=58.8 kJ/mol) would vaporize while…

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Q: Using the provided data, calculate the amount of heat, in kJ, required to warm 27.3 g of solid…

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Q: Calculate the heat required to convert 18.6 g of propyl alcohol, C3H8O, from a solid at -150°C into…

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Q: Liquid ethanol has a normal boiling point of 78.3 degrees celcius and has a heat if vaporization of…

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Q: 13.1 g OF liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants…

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Q: Heat was added to a 50.0 g sample of a liquid compound (molar mass = 87.9 g/mol), at a rate of 1.25…

A: Molar enthalpy of vaporization is the amount of heat required to convert one mole of liquid to its…

Q: Given the thermodynamic information below for ethylene glycol (molar mass = 62.068 g/mol): Normal…

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Q: Determine the normal boiling point of a liquid with vapor pressure 63.8 mmHg at 36.50°C, given that…

A: Accoding to Clausius Clapeyron equation,At normal boling point, the vapor pressure equal= 760 mmHg

Q: Determine the normal boiling point of a liquid with vapor pressure 63.8 mmHg at 36.50 degrees  C ,…

A: Given Information -  P1 = 63.8 mmHg T1  = 36.50 + 273 K = 309.50 K P2  = 760 mmHg T2  = ?  ∆Hvap =…

Q: calculate the quantity of energy in kj required to change 73.92 grams of liquid water at 38.8…

A: The liquid water is heated to raise the temperature from 38.8 to 100 degree Celsius. Then conversion…

Q: Determine the normal boiling point of a liquid with vapor pressure 63.8 mmHg at 56.50°C, given that…

A: Given: P1= 1 atm= 760 mm Hg P2= 63.8 mm Hg T2= 56.50°C= 56.50+273.15 K= 329.65 K ∆Hvap=43.5 kJ/mol…

Q: QUESTION 14 Which of the following E,Z designations are correct? Mark all correct answers. CO-H {Z}…

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Q: Calculate the heat energy released when 19.0 g of liquid mercury at 25.00 °C is converted to solid…

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Q: into

A: T1 = -151.0 °C T2 = 98.0 °C Tm =-117.3 °C Tb = 78.3 °C

Q: Consider the data in the table. Compound Melting point (°C) | AHfus (kJ/mol) Boiling point (°C) |…

A: The data given is,

Q: How much heat energy is required to convert 84.0 g (1.82 mol) of liquid ethanol (C2H5OH) at 78.4 °C…

A: Heat energy can be calculated by following formula:  q = m×s×(T2 - T1) Where m is the mass of the…

Q: Using the data shown below for water, determine in the following heating curve what region the water…

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Q: A 0.488 mol sample of liquid propanol (60.09 g/mol) is heated from 25.7°C to 329.2C. The boiling…

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Q: Calculate the heat energy released when 20.6 g of liquid mercury at 25.00 °C is converted to solid…

A: Given : Mass of mercury = 20.6 g Initial temperature of mercury = 25.00 oC = 273.15 + 25.00 = 298.15…

Q: Calculate the heat energy released when 25.4 g of liquid mercury at 25.00 °C is converted to solid…

A: The heat energy released for liquid to Solid state of a substance can be calculated by using…

Q: Suppose that 117.2 J of heat energy is required to completely vaporize 4.3 g of a pure liquid. If…

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Q: What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at…

A: We have to calculate the amount of heat needed.

Q: What amount of heat (in kJ) is required to convert 29.9 g of an unknown solid (MM = 67.44 g/mol) at…

A: The objective of the question is to calculate the total amount of heat required to convert a solid…

Q: How much heat is released ( in J) when 54.0 g of water at 10.0 °C is cooled to form ice at - 10.0…

A: Given the mass of water, m = 54.0 g  The initial state is water at 10.0 oC.  The final state is ice…

Q: A 21.3-g sample of ice at -14.6°C is mixed with 118.4 g of water at 80.0°C. Calculate the final…

A: Given: m1=mass of ice=21.3 gm2=mass of water=118.4 gT1=initial temperature=-14.6oCT2=final…

Q: The heat capacity, Cp, of liquid carbon disulfide is a relatively constant 78 J/(mol K). However,…

A: Solution In this question we use Third Law of Thermodynamics it tells us that as T → 0 K, S → 0.…

Q: How much heat is required to convert 87.1 g of acetone from a solid at –154.0°C to a liquid at…

A: •Mass of acetone(m)=87.1 gm  •Molar mass of acetone(mw) =58.08 gm/mol  •Mole (n) =m/mw = 87.1/58.08…

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: Using the provided data, calculate the amount of heat, in kJ, that must be removed to cool 29.6 g of…

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Q: The vapor pressure of a certain substance increases by 2.7 times as the temperature increases from…

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Q: 15) Liquid ammonia, NH3(1), was once used in home refrigerators as the heat transfer fluid. The…

A: The total energy required can be divided into three parts. The energy required to heat the liquid…

Q: Consider the following selected properties of water: Density (liquid water): d = 1.00 g/mL Heat of…

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Q: Lauric acid (C12H24O2) is 32.86 kJ/mol and enthalpy of ol. The melting point is 43.2°C. How much…

A: Given data are as follows Melting point =43.2 0C Heat capacity of solid= 2.15 J/g0C Heat capacity…

Q: The following information is given for antimony, Sb , at 1 atm: Boiling point = 1440.0°C   Heat of…

A: SOLUTION Mass of liquid antimony = 44.9 g Heat of fusion = 38.5 cal/g Energy removed = 38.5…

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

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Q: The normal boiling point of liquid acetone is 329 K. Assuming that its molar heat of vaporization is…

A: Given = Normal boiling point(T1)=329 k  Vaporization constant(∆Hv)= 29.0KJ/mol =29000J/mole External…

Q: 14. Calculate the amount of heat (in kJ) released when 35.0 g of benzene vapor is cooled from 96.0…

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Q: A certain monatomic substance has only one solid form, which melts at 190.2K and then remains liquid…

A: explanation

Q: What amount of heat (in kJ) is required to convert 20.0 g of an unknown solid (MM = 83.21 g/mol) at…

A: Given Molecular weight of solid = 83.21g/mol Mass = 20g specific heat capacity of solid = 2.39…

Q: Two 20.0 g ice cubes at -10.0 °C are placed into 265 g of water at 25.0 °C. Assuming no energy is…

A: Two 20.0 g ice cubes at - 10.0 °C are placed into 265 g of water at 25.0 °C .We have to calculate…

Q: Calculate the heat energy released when 26.9 g of liquid mercury at 25.00 °C is converted to solid…

A: Given: Mass of Hg = 26.9 g. Initial temperature of Hg = 25.00 oC = 298.15 K…

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.