Calculate the amount of heat required to completely sublime 99.0 g of solid dry ice (Co,) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ mol¬1. ? kJ Submit Request Answer

Q: how many kJ of energy are needed to change 20.8 g of ice at 0.00 °C to water at 20.31°C? use heat of…

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Q: Is dry ice evaporating  process exothermic or endothermic? Indicate the sign of ∆H.

A: Given: dry ice evaporating. The evaporation of dry ice requires input of heat energy.

Q: The heat of vaporization AH, of methanol (CH;OH) is 35.3 kJ/mol. Calculate th

A: If   vapourisation of methanol       CH3OH(l)     ⇔  CH3OH(g)    △Hv = 35.3 KJ/mol     then…

Q: What is the expected value for the heat of sublimation of acetic acid, in kJ/mol, if its heat of…

A: As we know that – According to Hess's law of constant heat summation, the heat absorbed or evolved…

Q: 6. A vapor volume of 1.17 L forms when a sample of liquid acetonitrile, CH3CN absorbs 1.00 kJ of…

A: Volume (V) = 1.17 L Boiling point= 81.6°C = 81.6 + 273 = 354.6 K Pressure (P) = 1.0 atm

Q: A sample of C₃H₄Br₂ has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for…

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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: The following information is given for silicon at 1 atm: Tb=2355.00°C Tm1410.00°C AHvap (2355.00°C)…

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Q: 3 How much heat energy is required to convert 200.0 g of ice at-20°C to all steam at 110°C at 1 atm?…

A: Water exists in three-phase solid, liquid and gas depending upon the temperature. Below 0oC water…

Q: Determine the total energy required to melt 1L of ice at -12°C to water vapor at a temperature of…

A: total energy required to melt 1L of ice at -12°C to water vapor at a temperature of 117°C

Q: How much energy (transferred as heat) is required to completely melt a 6.14 g sample of copper?…

A: Enthalpy of fusion - It is the energy required to change the state of a substance from solid to…

Q: The following information is given for bismuth at 1 atm:  = 1627.00°C   (1627.00°C) =  J/g  =…

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Q: is the heat reauired to melt 51.8 of solid benzene, Cati at its melting. pent? ....

A: The mass of Benzene = 51.8 g To Calculate the heat required to melt the solid Benzene we required…

Q: 4. the vapor pressure of a liquid is equal to the atmospheric pressure.: a. boiling increase. b.…

A: All the given questions are answered.

Q: Find ΔHrxn, ΔSrxn, and ΔGrxn for this phase change CCl4 (l)    CCl4 (g)      and then,    what…

A: The reaction taking place is given as, => CCl4 (l) -------> CCl4 (g)

Q: n statement describes the relationship between the attractive forces among particles and the boiling…

A: Molecular attractive forces such as vanderwaals force, London force, dipole interactions, hydrogen…

Q: Using the data below, determine how much heat (in Joules) is required to convert 405.0 g of ice at…

A: we have to calculate the heat needed for the given conversion

Q: 11.4 If 42.0 k of heat is added to a 32.0-g sample of liquid meth- ane under 1 atm of pressure at a…

A: GivenThe total heat transferred = 42.0kJPressure= 1 atmMass= 32.0gT= -170 °Cc1= 3.48 J/gKc2=…

Q: The organic compound n-pentane, C5H12, boils at 36.1°C. 1st attempt What is its molar heat of…

A: Given: Normal boiling point of pentane = 36.1 oC And vapor pressure at 20 oC = 541 torr.

Q: Chloroform, CHCl3, a volatile liquid, was once used as an anesthetic but has been replaced by safer…

A: The question is based on the concept of boiling. we have to identify the vapour pressure at the…

Q: Q2) If AH°¡ of H2O@ is -285.8 kJ/mol and AH°f of H2O is -241.8 kJ/mol, then the AH° of vaporization…

A: Given: ∆Hºf( H2O(l))= -285.8 KJ/mol ∆Hºf( H2O(g))=-241.8 KJ/mol The vaourization process occurs as…

Q: Calculate the heat exchange (in kJ) involved in the conversion of 27.64 g of solid acetone, C3H60 at…

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Q: The enthalpy of fusion (ΔHfusion) for a substance is +7 kJ, while the enthalpy of sublimation (…

A: Fusion is the process of converting solid into liquid (i.e molten form)  And vaporization is a…

Q: Substance C4H10O has enthalpy of vaporization ∆Hvap = 26.5 kJ/mol and M = ____ g/mol. When 22 g of…

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Q: Consider the heating curve provided for 1.00 mole of a substance that begins as a solid at -14.8 °C…

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

Q: What is the quantity of heat (in kJ) associated with cooling 150.3 g of water from 25.60°C to ice at…

A: Given data mass of water : m=150.3 g Initial temperature of water : T1=25.60 °C Melting temperature…

Q: How much energy (kJ) is needed to heat 25.0 g of isopropyl alcohol from -25.0°C to +90.0°C? Molar…

A: we have to calculate the energy needed to heat isopropyl alcohol

Q: Find the temperature in °C of a sponge of heat capacity C=1.859 kJ/°C, initially at 35.4 °C, after…

A: To calculate the amount of heat released by a sponge, the equation used is: q=C × T2-T1…

Q: Consider the given phase thermochemical data for compounds A and B. Which of the following…

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Q: The following information is given for water at 1 atm: AHvap (100.00°C) = 2.259 × 10³ J/g AĦfus…

A: The amount of heat required to raise the temperature of solid water from 258 K to 273 K can be…

Q: Question 14 of 34 Submit What quantity of heat, in kJ, is required to convert 50.0 g of ethanol…

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Q: For liquid  CH3OH a plot of log natural of vapor pressure against the reciprocal of absolute…

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Q: pts 2req Use the References to access important values if needed for this question. The following…

A: Molar mass of benzene = 78.11 gram   so, 41.4 gram of benzene = (41.4/ 78.11) mol = 0.530 mol…

Q: A heating curve of one gram of a pure solid at 1 atm is shown to the right. Which factor affects the…

A: A pure solid is heated. In the given heating curve, Segment AB represents all solid (heat is…

Q: Given that  q = n · ΔHfus,  how many moles of water are present if 53.4 kJ of heat are required to…

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Q: The enthalpy change in water for converting 1 mol of ice at -50 degrees Celsius to water and 80…

A: First the ice at -500C is converted to melting point. The mass of ice is also calculated as follows,

Q: Calculate the energy in Joules required to convert 72 g of ice originally at -15°C into steam at…

A: Given : Mass of ice = 72 g Ice originally at -15°C to steam at 105°C To find : Energy in joules…

Q: When 2 g of solid A, at its melting point of 34.0 °C, was added to 62.7 g of liquid A at 51.2 °C,…

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Q: The freezing point of a pure liquid involves equilibrium between molecules in the liquid state and…

A: Freezing point is  nothing but the temperature at which pure liquid phase is converted to solid…

Q: A 31.0 gram block of an unknown metal at 88.0 °C was dropped into an insulated flask containing…

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Q: Calculate the heat absorbed when 117 g of liquid ethanol at 25.0°C is converted to gaseous ethanol…

A: The heat absorbed in the above process is given by  Q = m X Cl X ΔTl + ΔHvap X n + m X Cg X ΔTg…

Q: The heat of vaporization of water at 373 K is 40.7 kJ/mol. Find q,w, ∆E, and ∆H for the evaporation…

A: The heat of vaporization is defined as the quantity of heat required to convert 1g of a liquid into…

Q: A 46.20 g sample of liquid aluminum at 877.0 °C is poured into a mold and allowed to cool to 29.0…

A: Total heat released is sum of heat released in every step of the cooling

Q: kJ and its normal boiling point is -66. °C. Calculate the vapor mol The enthalpy of vaporization of…

A: To calculate the value of Vapor pressure at given temperature , we would use Clausius Clapeyron…

Q: Q3) a) The following information is given for water, H2O, at 1atm: boiling point = 100 °C…

A: (a) Given that : At 1 atm, boiling point = 100 °C Hvap(100 °C) = 40.7 kJ/mol specific heat…

Q: Determine the heat involved when an 80.0 g ice at - 5 °C is converted to steam at 120 °C? Cr of ice…

A: (1.)  Determine the heat required to raise the temperature of the ice from −5 0C to 0 0C : q1 = m ×…

Q: melting point boiling point 0.0°C 100.0°C 2.05 J/g.°C 4.184 J/g °C 2.02 J/g °C 6.02 kJ/mol specific…

A: Mass of water = 16.6 g Water temperature = 80 oC Specific heat of water = 4.184 J/mol.oC   Mass of…

Q: Use the References to access Important values if needed for this question. The following information…

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

Q: What intermolecular force(s) must be overcome to perform the following? (a) melt ice (b) sublime…

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Q: Identify the areas/points in the following phase diagram. 1,000+ 800 P (torr) 600 400 200 -10 10 20…

A: A phase diagram is a graph which shows under what conditions of temperature and pressure distinct…

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.