Using standard enthalpies of formation and standard molar entropies, determine the normal boiling point of methanol, CH3OH

Q: Calculate  ΔH⁰298   (in kJ) for the process P(s) + 5/2 Cl2(g) → PCl5(g) from the following…

A: Given,

Q: How Gibbs free energy is determined by the volume of the substance ?

A: To find: relation between Gibbs free energy and volume?

Q: Methylhydrazine (N2H3CH3) is a common liquid propellant used in rocket fuels. Look for the standard…

A: We are said to look for standard enthalpies of formation of reactant and product.  Enthalpy of…

Q: The enthalpy of vaporization of chlorine at the standard (1 atm) boiling point (284 K) is 20.41…

A:

Q: SCl4(g) + 2 O2(g) ΔHo = 40.2 kJ/mol and ΔSo = 132.3 J/K.mol. What is the equilibrium constant for…

A:

Q: The evaporation enthalpy of benzene C6H6 is 394.0 J / g at the normal boiling point which is 80.10…

A: Given : Enthalpy of vaporisation of benzene = 394.0 J/g Boiling point temperature = 80.10 oC And…

Q: Given that: ΔHof [NO2(g)] = +34.0 kJ mol−1 ΔHof [NO(g)] = +90.0 kJ mol−1 What is the standard…

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Q: Calculate "work" and "change in internal energy" for the conversion of three moles of ethanol at 78…

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Q: From the following enthalpies of reaction find ΔHrxn for 2 HCl(g) + F2(g) ---> 2 HF(l) + Cl2(g):  4…

A: Given, 4 HCl(g) + O2(g) ---> 2 H2O(l) + 2 Cl2(g); ΔH = -148.4 kJ/mol1/2 H2(g) + 1/2 F2(g) --->…

Q: A 0.502 g sample of liquid C6H12 was combusted using excess oxygen gas inside a bomb calorimeter,…

A:

Q: The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ/mol. What is the ΔH at 373…

A:

Q: The combustion of 2.295 g of propanol (C3H7OH) increases the temperature of a bomb calorimeter from…

A: Heat of Combustion- Is the measure of the amount of heat released when one mole of a substance is…

Q: The enthalpy for the combustion reaction of solid cysteine, C3H7NO2S, resulting in the gases CO2,…

A: Answer: This question is based on first law of thermodynamics according to which: ∆U=∆H-∆ngRT Here:…

Q: Use standard enthalpies of formation to calculate ΔH° for the following reaction. MgCO3 (s) + 2HCl…

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Q: Calculate the ΔH for the reaction: C2H4 (g) + H2 (g) --> C2H6 (g), from the following data:   C2H4…

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Q: nitial temperature of a reaction is 10.0oC. When temperature increases to 20.0oC, the equilibrium…

A: we know ln k2k1=∆HR1T1-1T2where , k2= final rate constant                k1=Initial rate constant…

Q: When 2.18 g of copper(II) chloride (CuCl2) is dissolved in 119 g of water in a styrofoam calorimeter…

A:

Q: Find ΔH for the combustion of ethanol (C2H6O) to carbon dioxide and liquid water from the following…

A: First calculate the change in temperature. Calculate the heat of bomb calorimeter is as follows,

Q: CO (g) + 2 O₂ (g) → CO₂ (g) a) For this gas phase reaction, determine (i) ArxnH (in kJ/mole) and…

A: (A)The value of delta H for the given reaction can be calculated as ∆Hf = ∑Hproducts - ∑H reactants=…

Q: Mg(s)  +  2HCl(aq) → MgCl2(aq)  +  H2(g) The temperature increases from 23.00 to 33.10 °C as a…

A:

Q: The molar heat capacity at constant pressure for CO2 is 36.61 J mol-1 K-1. How much heat in J is to…

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Q: The standard enthalpy of combustion of solid carbon to form carbon dioxide gas is -393.7 kJ per mol…

A:

Q: The combustion of 2.474 g of propanol (C3H7OH) increases the temperature of a bomb calorimeter…

A:

Q: The enthalpy of vaporization of ammonia is 23.35 kJ/mol at its boiling point (–33.4°C). Calculate…

A: Given: Enthalpy of vaporization of ammonia = 23.35 kJ/mol. Boiling point of ammonia = -33.4 oC And…

Q: Using the tables, what is the standard Gibbs free energy change for the following reaction? 2 Cu (s)…

A:

Q: When 4.20 g of solid NH4NO3 dissolves in 50.0 g of water at 26.8°C in a calorimeter, the temperature…

A: The heat of a substance is given as:

Q: Calculate ΔH for this reaction N2H4 (l) + O2 (g) → N2 (g) + 2H2O (l) given the following data:…

A:

Q: (d) What is the sign of the standard reaction ENTROPY? Does the entropy provide a favorable or…

A: The equilibrium reaction given is, =>

Q: The molar heat capacity at constant pressure for CO2 is 36.61 J mol-1 K-1. How much heat in J is to…

A: To solve this problem first we will calculate the mole of CO2  then amount of heat released will be…

Q: A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter,…

A: Given, mass of the sample is 0.576 g of liquid C5H12  Heat capacity of calorimeter is 4.957 Kj/°c…

Q: In the decomposition of H2O2(l) to H2O(l) and O2(g) the resulting ΔSuniv is 454.3 J/K; a spontaneous…

A: True, the decomposition of H2O2(l) to H2O(l) and O2(g) the resulting ΔSuniv is 454.3 J/K; a…

Q: From the following enthalpies of reaction find ΔHrxn for 2 HCl(g) + F2(g) ---> 2 HF(l) + Cl2(g): 4…

A: The main reaction is – 2HCl g + F2g →2HFl + Cl2g

Q: NO3KNO3 is dissolved in 229 g of water at 23.00 °C.   KNO3(s)−→−−H2OK+(aq)+NO−3(aq)   The…

A:

Q: Suppose we redefine the standard state as P=4bar. Find the new standard ΔfG∘ values of the following…

A: The objective of the question is to find a new standard value of HCl (g) at pressure .Given, at bar…

Q: The molar heat capacity Cp,m of SO₂ (g) is described by the following equation over the range 300 K…

A:

Q: A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter,…

A: Explanation The heat of reaction, ΔrU is  calculated as: ΔrU = ΔU / n Where ΔU is the change in…

Q: 1.6 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A:

Q: The normal boiling point of benzene is 80 °C. At 100 °C and 1 atm, which term isgreater in magnitude…

A:

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.