Five cubic meters of a 1.00-molar aqueous sulfuric acid solution (SG = 1.064) is stored at 25°C. Use data in Tables B.1 and B.l1 to calculate the standard heat of formation of the solution in kJ/mol H2SO4relative to the solute elements and water, and the total enthalpy of the solution relative to the same reference conditions.
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- 50.0mL of 0.300M CuSO4 is mixed with equal volume of 0.400M. The reaction temperature raised by 3.20oC. a) Determine the molar enthalpy of reaction. 2 NaOH + CuSO4 à Cu(OH)2 + Na2SO4 b) Write a thermochemical equation (with enthalpy value embedded in the equation) to represent the reaction:arrow_forwardSuppose that 4.65 grams of X (MW = 25.94) are dissolved in 536 mL of water, and the water temperature changes from 22.65°C to 23.57°C. Assume that the mass of X is negligible compared to the mass of the water. Assume the specific heat of water is 4.2 J/(g.°C) and the density of water is 1.0 g/mL. Calculate the enthalpy of dissolution of X in kJ/mol. Report your answer to three decimal places.arrow_forwardA coffee cup calorimeter with a heat capacity of 7.40 JrC was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AGNO, was mixed with 50.0 mL of 0.310 M KBr. After mixing, the temperature was observed to increase by 3.04 °C. Calculate the enthalpy of reaction, AHan, per mole of precipitate formed (AgBr). Assume the specific heat of the product solution is 4.11 J/ (g C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO, and KBr. theoretical moles of precipitate formed from AgNO,: moles theoretical moles of precipitate formed from KBr: moles Calculate the heat change experienced by the calorimeter contents, qontents -arrow_forward
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- using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?arrow_forwardThe first and second ionization enthalpies of calcium.Ca, are 596 kJ mol-1 and 1145 kJ mol-1 respectively at 25 °c.Calculate the standard enthalpy change for the processCa(g) → Ca2+(g) + 2e- (g) at this temperature.arrow_forward4.00 g NaOH(s) (39.996 g mol–1) dissolves in 100.0 g of water in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The density of the solution is 1.00 g cm–3. The heat of dissolution is –44.51 kJ mol–1. The specific heat of the solution is 4.184 J g–1 °C–1. The specific heat of the calorimeter is 100 J °C–1. What is the final temperature of the solution? 30.23°C 25.94°C 28.32°C What is the energy lost to the calorimeter? 579 J 832 J 721 Jarrow_forward
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- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
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