A certain hydrocarbon of the molecular formula CxH2x has a standard enthalpy of formation ∆Hf° = –115.0 kJ/mol and a standard enthalpy of combustion ∆H°combust = –5319.4 kJ/mol. What is x? Use the following data: ∆Hf°[CO2(g)] = –393.5 kJ/mol, ∆Hf°[H2O(l)] = –285.8 kJ/mol.

Q: Consider the reaction shown below and the tabulated thermochemical data at 298 K. Which of the…

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Q: 1. In which of the following cases do you observe a spontaneous process? А. AS = 10 J/K, AS =-10 J/K…

A: We are authorised to solve only one question at a time. Since you have not mentioned, we are solving…

Q: Calculate ΔHf for HCN(g) at 25°C, given the following related reaction at 25°C,  2 NH3(g) + 3 O2(g)…

A: given, 2 NH3(g) + 3 O2(g) + 2 CH4(g) → 2 HCN(g) + 6 H2O(g); ΔHrxn = -870.8 kJ ΔHf = -80.3 kJ/mol for…

Q: Consider the following reaction and the tabulated thermochemical data at 298 K. Substance 4 NH AH°…

A: Standard entropy is the entropy of one mole of a substance at a temperature of 298 K and a pressure…

Q: Given the following thermochemical equations, C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l) ∆H = -1299.5 KJ…

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Q: The heat of combustion of fructose, C6H12O6, is -2812 KJ/mol. If a fresh golden delicious apple…

A: Molar mass of fructose = 180.16 g/mol

Q: (Q71) Consider the hydrogenation of ethene to form ethane that occurs according to the following…

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Q: The U.S. requires automobile fuels to contain a renewable component. The fermentation of glucose…

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Q: Calculate the standard heat of formation, ΔHfo, for FeS2(s), given the following information:…

A: Given, ∆Hf = ? 2FeS2(s) + 5O2(g) → 2FeO(s) + 4SO2(g) ∆Hrxn = -1370 kJ ∆Hf for SO2(g) = -297 kJ/mol…

Q: Given the thermochemical expression below: CaO (s) + 3C (s) ----> CaC2 (s) + CO (g)…

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Q: Calculate ΔH° for the combustion of methane. CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) Given the…

A: We have to calculate the ∆H° for Reaction.

Q: 3. Compounds with carbon-carbon double bonds, such as ethylene, C,H,, add hydrogen (H,) in a…

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Q: (Q73) If both the enthalpy change and the entropy change for a certain process have negative values,…

A: We know that ∆G=∆H-T∆S Where ∆G is gibbs energy. ∆H is enthalpy chnagr and ∆S is entropy change  For…

Q: combustion of octane (in gasoline) occurs according to the reaction 2 CgH₁8 + 25 0₂ 16 CO₂ +18 H₂O.…

A: Given-> ∆Hf(octane) = -268.8 KJ/mole ∆Hf(CO2) = -394KJ/mole ∆Hf(H2O) = -286 KJ/mole

Q: Br () H Pd on C (a) () NANO, HCI, 0-5 °C () CUCN NO2 KMno, (b) heat Pd(OAc), PPh, (c) -B(OH Na,Co,…

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Q: A 1.72 g sample of the saccharide, C6H1206, shown below is combusted in a constant volume…

A: By the estimate of the enthalpy of reaction by looking at the individual bonds involved. If we know…

Q: Given that that AH of formation of n-butane. J: C-H - 412, C-C-340, H-H- 436, AH ab kl graphite:…

A: Interpretation-  To determine the enthalpy of formation of n- butane when here given ∆HoB.D / KJ :…

Q: Calculate ∆Gº for the reaction, 2SO2(g)+O2(g)→2SO3(g), where ∆Gfº= -300 kJ/mol for SO2(g) and -370…

A: Gibbs Free Energy for a reaction is calculated by subtracting  the Gibbs energy of formation of…

Q: W(s) W(1) AH fu = 35 kJ/mol; AS" fus = 10 J/(mol K) The chemical equation and thermodynamic data for…

A: Introduction :  We have to tell that the tungsten will melt or not .

Q: When 1942 J1942 J of heat energy is added to 41.9 g41.9 g of ethanol, C2H6O,C2⁢H6O, the temperature…

A: Using the relation Q = mCΔT we can find molar heat capacity of C2H6O.

Q: The specific heat capacity of ethanol (C₂H5OH) is 2.44 J/g. K. What is its molar heat capacity (in…

A: Here we are required to find the molar heat capacity of ethanol

Q: Calculate AHxn for the reaction: 2H,0(1) → 2H2(g) + O2(g) Use the following information: H,0(g) →…

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Q: 2) Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction:…

A: Given, a) N2(g) + O2(g) ➝ 2NO(g)  ∆H°rxn = +183 kJ b) 1/2N2(g) + O2(g) ➝ NO2(g)  ∆H°rxn = +33 kJ…

Q: Q2.) For a particular reaction, ΔH = -32 kJ and ΔS = -90 J/K . Assume that ΔH and ΔS do not vary…

A: Given : ΔH = -32 kJ  ΔS = -90 J/K 1) To calculate Temperature at which  ΔG=0  ΔG = ΔH  - TΔS ΔG=0…

Q: At constant volume, the heat of combustion of a particular compound is –3639.0 kJ/mol. When 1.471 g…

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Q: What is the standard enthalpy of formation of CaCO3(s)? CaO(s) + CO2(g)  →  CaCO3(s); ΔH° = -179.4…

A: The given data is as follows: CaO(s) + CO2(g) → CaCO3(s)                   ∆H°=-179.4 kJ/mol The…

Q: What is the change in internal energy (in kJ/mol) of the given reaction if 2 moles of sulfur dioxide…

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Q: Isooctane (C8H18; density = 0.69 g/mL) is one of the many hydrocarbons that make up gasoline. Use…

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Q: (a) Consider the following chemical reaction: 3Fe2O3(s) + CO(g) → 2Fe3O4(s) + CO2(g) ΔH = ? Use…

A: Given: The thermochemical data, 4Fes + 3O2g → 2Fe2O3s                      ∆H° = -1652 kJ/mol…

Q: 2.2 Methanol can also be combusted in the presence of oxygen in order to release its energy. 5.24 g…

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Q: The thermochemical reaction equation for photosynthesis is as follow: 6H2O (l) + 6CO2 (g) → C6H12O6…

A: Solution:     The endothermic reaction shows the energy absorbed during the chemical reaction while…

Q: 2. Give an example of an endothermic process that is spontaneous b. an exothermic process that is…

A: Spontaneous process :-          It is a process, in which process occurs without any external input…

Q: The heats of the following reactions at 25°C are: Na(s) + 1/2Cl,(g) → NaCl(s) AH° = - 98230 cal…

A: The heat of the reaction is the energy that is released or absorbed when chemicals compounds are…

Q: 11.Describe the conditions at which the following thermochemical equations are  spontaneous. If you…

A: Chemical Reaction are almost invariably accompanied by energy changes which ordinarily, appear in…

Q: Given the following chemical reaction occurring in a 2.00 L container: A (g) + 2 B(s) ↔ 4 C(g) + 3…

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Q: When 0.515 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises…

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Q: What is the change in internal energy (in kJ/mol) of the given reaction if 2 moles of sulfur dioxide…

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Q: Given the following thermochemical equations, C2 (g) +5/2O2 (g) → 2CO2 (g) +H2O (l) ΔH = −1299.5kJ…

A: Given: C2H2(g)+52O2(g)→2CO2(g)+H2O(l)     ∆H=-1299.5 kJ---eqn(1)C(s)+O2(g)→CO2(g)…

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: Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of…

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Q: Consider the decomposition of liquid benzene, C6H61l2, togaseous acetylene, C2H21g2:C6H61l2 ¡ 3…

A: Decomposition reactions are one in which the reactants get splits into one or more than one…

Q: (Q77) The standard Gibbs free energy (AG°rxn) for the formation of sulfur trioxide from sulfur…

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

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Q: Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): ⅓C6H6(l) --->…

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Q: For the reaction 2 A(g) → A2(g), Q = -20.00 kJ for the formation of one mole of A2(g) at constant…

A: Given data: The reaction is- 2 A(g) → A2(g), Q = -20.00 kJ  Temperature = 25.00◦C

Q: Calculate ΔH°rxn

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Q: Calculating ΔG under Nonstandard Conditions What is the free energy change for the process shown…

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Q: Calculate the molar heat capacity of C6H14

A: Given :-  mass of hexane = 45.9 g  heat = 1786 J  change in temperature = 17.2 °C To calculate :-…