Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 3.45 g of sucrose is combusted in a constant volume (bomb) calorimeter, 56.9 kJ of heat is liberated. Calculate ΔE for the combustion of 8.95g of sucrose. Calculate ΔH for the combustion of 8.95 g of sucrose

Q: In a constant‑pressure calorimeter, 65.0 mL of 0.350 M Ba(OH)2 was added to 65.0 mL of 0.700 M HCl.…

A: Given:65.0 mL of 0.350 M Ba(OH)265.0 mL of 0.700 M HCl.Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

Q: Determine ΔH for the third reaction from the information given. S(s) + O2(g) ↔ SO2(g) ΔH = -296.1…

A: Given;

Q: What is the ΔSo for the combustion reaction of ammonia NH3(g) to nitrogen dioxide NO2(g) and water…

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Q: THERMODYNAMICS: A 1.61 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

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Q: Why do elements always have ΔH∘f=0? a) The standard state of elements is the reference point for…

A: •Given:- Here is question is asking that why ∆H°f always zero for elements.

Q: Calculate ΔH of a piece of metal with a specific heat of 0.98 J /g°C and a mass of 460g which is…

A: Thermodynamics is branch of chemistry in which we deal with amount of heat evolved or absorbed by…

Q: Find the ΔH (in kilojoules) for the reaction below, given the following reactions and subsequent ΔH…

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Q: Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene…

A: Given data,Mass of naphthalene=1.025gInitial temperature=24.25oCFinal…

Q: Calculate the work (w) and ΔEo, in kJ, at 298 K and 1 atm pressure, for the combustion of one mole…

A: Given-> ∆H° = -3169.3 KJ/mole T= 298 K P =1 atm

Q: Calculate ΔHrxnfor the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions…

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Q: Calculate ΔrHΔrH for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions…

A: 1- First reverse the Last equation : 2CaO(s) ------> 2Ca(s) + O2(g)..... (4)  ∆H1 = +1269.8…

Q: 1. A gas is confined to a cylinder under constant atmospheric pressure. When 0.49 KJ of heat is…

A: Heat Heat is the result of the movement of kinetic energy within a material or an item, or from an…

Q: Given: C6H12O6 (s) + 6 O2 (g) → 6CO2 (g) + 6 H2O (liq) When 3.500 g of glucose, C6H12O6 (MW =…

A: Burning of glucose to give gaseous carbon dioxide and liquid water is an exothermic reaction.In an…

Q: When 0.596 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises…

A: Mass of biphenyl =0.596 g Change in Temperature(T) = 30.4°C —26.4°C = 4.0°C heat capacity of the…

Q: When 50.0 mL of 0.987 M H2SO4 is added to 25.0 mL of 2.00 M NaOH at 25.0 °C in a calorimeter, the…

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Q: Calculate ΔSº for the reaction using the data table provided. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)…

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Q: 25.0 mL of 1.00 M HCl at 23.5oC react with 25.0 mL 1.00 M NaOH in a styrofoam calorimeter whose…

A: The energy of a system is always conserved. The amount of heat released or absorbed by the reaction…

Q: give 2 examples of enthalpy, entropy, and Gibbs free energy.

A: Examples of enthalpy, entropy, and Gibbs free energy are given below

Q: When a 4.50-g sample of liquid octane (C8H18) burns in a bomb calorimeter, the temperature of the…

A: Mass of octane = 4.50 g  Temperature change = 27.5 ∘C Heat capacity of calorimeter = 6.27 kJ/∘C

Q: using the standard molar enthalpies of formation here below. Give the answer in kJ/mol-rxn (write…

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Q: Use the information provided to determine ΔH°rxn for the following reaction: 3 A(s) + B(g) → 2 X(s)…

A: The standard enthalpy of the given reaction is calculated is follows :

Q: Calculate ΔHrxn for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and…

A: "Hess law" helps in the evaluation of enthalpy change (Delta H)  for any specific reaction. When the…

Q: 50.0 mL of 1.00 M HCl(aq) and 100.0 mL of 1.00 M NaOH(aq), both at 25.0oC, are added together in a…

A: Total volume of the solution, (V) = (50 + 100) mL = 150 mL. The density of the solution, d = 1 g/mL.…

Q: The following reaction was performed in a constant volume bomb calorimeter: 2N2O(g)  +  3O2(g)   →…

A: Given:  Delta H = -31.7 KJ /°C  Delta T = 0.385 °C  Heat capacity = 5.16 KJ/°C

Q: A system does 531531 kJ of work and loses 286286 kJ of heat to the surroundings. What is the change…

A: Work done by the system = 531531 KJ Loses heat to sorroundings = 286286 KJ  Change in Internal…

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

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Q: A 0.656-g sample of acetylsalicylic acid (C9H8O4) is burned in a bomb calorimeter and the…

A: The objective of this question is to calculate the change in energy (ΔE) for the combustion reaction…

Q: oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC,…

A: Heat(q) = m.c..□T Using energy conservation,  Heat loss by Acid = Heat gain by water + Calorimeter…

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: A 90.0 mL sample of 0.200 M NaOH is mixed with a 90.0 mL sample of 0.200 M HNO3 in a coffee cup…

A: Volume of NaOH = 90.0 mLConcentration of NaOH = 0.200 MVolume of HNO3 = 90.0 mLConcentration of HNO3…

Q: the

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Q: When 1.045 g of K2O is added to 50.0 mL of water at 25.0 ∘C in a calorimeter, the temperature of the…

A: Information of question

Q: When 2.25 g of sodium hydroxide (NaOH) was dissolved in 100.00 g of water a value of 10.00oC was…

A: The heat of the solution produced when 2.25 g of sodium hydroxide is dissolved in 100 g of water, is…

Q: THERMODYNAMICS: A 1.98 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A: Given the mass of acetic acid (HC2H3O2) sample taken = 1.98 g Since the temperature of the…

Q: 5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the…

A: The question can be solved by giveb formula,  Q=m×C×dT where Q = heat energy (Joules, J),  m = mass…

Q: The enthalpy change for the following reaction is -36.2 kJ 2A(s) + B(g) → C(g) Determine the ΔH…

A: Answer:- This question is answered by using the simple concept of Hess law of constant heat…

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

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Q: The combustion reaction of 1-pentanol is: C5H11OH(l)+152O2(g)→5CO2(g)+6H2O(l) The heat of…

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Q: Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 1.43 g of…

A:

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

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Q: 1.87 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The…

A: Mass of acetic acid = 1.87g Molar mass of Acetic acid = 60g/mol Heat capacity of calorimeter =…

Q: reagents inside a simple calorimeter. The outside of the calorimeter is made of an aluminum cup with…

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Q: The standard enthalpy change for the combustion of 1 mole of propane is –2043.0 kJ.         C3H8(g)…

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Q: When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid…

A: Enthalpy of reaction , ΔH can be calculated as : ΔH =  Sum of Enthalpy of formation of product - Sum…

Q: Given the following data, calculate ΔH for the reaction of two moles of carbon monoxide with oxygen…

A: The indirect calculation of enthalpy change by use of several reactions with known enthalpies is…

Q: Both a coffee-cup calorimeter and a bomb calorimeter can beused to measure the heat involved in a…

A: The amount of heat required to raise the temperature by 1∘C is termed as heat capacity.

Q: Use ΔH formation information provided to calculate ΔH of the reaction (in kJ) for the following:…

A: In this question, we have to find out the correct answer of given problem by the help of Enthalpy…

Q: If we measure the heat change (q) of everything in a system except the calorimeter, we can use the…

A: Given: mass of hot water = 5.59 g mass of cold water = 5.62 g C = 4.186 J/g°C Temperature of hot…

Q: calculate ΔE for the combustion reaction per mole of xanthone burned (kJ/mol).

A:

Q: THERMODYNAMICS: A 1.87 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb…

A: