21.0°C to 27.5°C. calculate the enthalpy change for the reaction in kJ/mol HCl, assuming that the calorimeter

Q: Suppose that the reaction of 2.172 moles consumes 3.21 kJ of heat. What is the molar enthalpy of the…

A: The answer to the following question is :

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Q: A scientist measures the standard enthalpy change for the following reaction to be 74.8 kJ: 2HBr(g)…

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Q: Suppose that the reaction of 1.116 moles consumes 30.34 kJ of heat. What is the molar enthalpy of…

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Q: Iculate föllowing. aicate if the system do work on the surroundings or the surroundings do work on…

A: Hi! there, since there are multiple questions posted. We are answering first question. If you need…

Q: A 35.0 mL solution of 0.600 M compound A is mixed with an excess of compound B solution at 12.8 C in…

A: Since the temperature of the solution inside the calorimeter is increased, heat is absorbed by the…

Q: If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup…

A: Given : mass of MgO reacting = 1.85 g Initial temperature of solution = 21.3 °C Final temperature of…

Q: Suppose that the reaction of 2.553 moles produces 38.34 kJ of heat. What is the molar enthalpy of…

A: Let us consider a reaction,          Reactant -----> Product    The values provided in the…

Q: A 1.96 g sample of titanium was burned in a bomb calorimeter. The bomb calorimeter has a heat…

A: The solution is as follows :

Q: Define calorimetry and describe two commonly used calorimeters. In a calorimetric measurement, why…

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Q: When 150 mL of 1.00 M NaOH is added to 100 mL of 1.30 M HCl in an insulated calorimeter, the…

A: To calculate the enthalpy change for the neutralization reaction, the following quantities are…

Q: A 0.1694 g sample of benzopenone(C13H10O) is burned in a bomb calorimeter that has a heat capacity…

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Q: 8. The reaction below was carried out in a calorimeter initially at 22.0 °C. After 0.0180 g of iron…

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Q: In the laboratory, a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used…

A: qw = - qTin mw × cw × (Tf - Ti) = - { mtin × ctin × (Tf - Ti) On substituting the values into it, we…

Q: When 1.23g C6H6(l) are burned, 51.5KJ of heat are released.  Calculate the enthalpy for this…

A: Heat of formation of the compound can be calculated from the reaction and enthalpy of the reaction .…

Q: 3. When a student mixes 50 mL of 1.0 M HCI and 50 mL of 1.0M NaOH in a coffee- cup calorimeter, the…

A: given - 50 ml of 0.1 HCl  50 ml. of 0.1 NaOH density = 1 g/ml specific heat = s = 4.18 J/g K initial…

Q: 5.00 – mL of 0.64M HCl and 45.00 – mL 0.77M NaOH, both initially at 26.0°C, are mixed in a…

A: Given: Concentration of HCl = 0.64 M Concentration of NaOH = 0.77 M Volume of NaOH solution added =…

Q: A student performed the procedure described in the lab manual using 49.9 mL of 1.0 M HCI and 49.3 mL…

A: Molarity of HCl = 1.0 MVolume of HCl: 49.9 mLMolarity of NaOH = 1.0 MVolume of NaOH = 49.3 mLInitial…

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A: (a).

Q: 2CH3OH(g)→2CH4(g)+O2(g),ΔH=+252.8 kJ   For a given sample of CH3OH, the enthalpy change during the…

A: Given,For a sample of CH3OH, the enthalpy change during the reaction is 82.9 kJ.

Q: Given the following two reactions and their enthalpy changes,             2 ClO2 (g)   -->   Cl2…

A:

Q: Consider this combination reaction: 2Mg(s)+O2(g)→2MgO(s); ΔH= −1204 kJ What is the enthalpy for the…

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Q: The standard enthalpies of combustion (ΔH°comb) of C6H6(g) and C2H2(g) are –3301 kJ/mol and –1300…

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Q: Mg(s)+2H2O(l)→Mg(OH)2(s)+H2(g). Calculate the standard enthalpy change for this reaction. Calculate…

A: Enthalpy change of the given reaction can be calculated for the given formula.

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Q: Cold packs are made from ammonium nitrate and water. To measure the enthalpy of this reaction 2.50…

A: Given information,    Mass of solution = 50.0 g    Temperature change = 25.8 - 21.9 = 3.9oC.…

Q: A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The…

A: Given data:Calculate the heat evolved in the reaction of HCl and NaOH and enthalpy of…

Q: If a reaction causes 25.0 g of water to decrease temperature by 14.24 oC at constant pressure, what…

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Q: When HCl(aq) and NaOH(aq) are mixed in a beaker, the beaker feels warm to the touch. What is known…

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Q: When 10.00 g of phosphorus is burned in O2( g) to form P4O10(s), enough heat is generated to raise…

A: Given; M = 10.0 g c = 4.2jgC ∆T = (38-18)oC

Q: A 77.5g piece of brass is heated so that its temperature is 98.7◦C. Next, it is quickly placed in a…

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Q: The combustion of 0.1559 g benzoic acid increases the temperature of a bomb calorimeter by 2.52°C.…

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Q: 150.0 mL of dilute hydrochloric acid is placed in a coffee cup calorimeter. The initial temperature…

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Q: The combustion of 0.1584 g benzoic acid increases the temperature of a bomb calorimeter by 2.54°C.…

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Q: A scientist measures the standard enthalpy change for the following reaction to be 209.4 kJ : CHĄ(g)…

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Q: When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter…

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Q: An exothermic reaction liberates 7.58 kJ of heat in a coffee cup calorimeter containing 157 grams of…

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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.