When 21.9 mL of 0.500 M H2SO4 is added to 21.9 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50 °C, thetemperature rises to 30.17 °C. Calculate AH of this reaction. (Assume that the total volume is the sum of the individualvolumes and that the density and specific heat capacity of the solution are the same as for pure water.) (density for water= 1.00.) Be sure your answer has the correct number of significant figures.mLNote: Reference the Phase change properties of pure substances table for additional information.kJmolx105E

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Answered: When 21.9 mL of 0.500 M H2SO4 is added…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =
When 28.7 mL of 0.500 M H₂SO4 is added to 28.7 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50 °C, the temperature rises to 30.17 °C. Calculate AH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the g same as for pure water.) (density for water = 1.00 .) Be sure your answer has the correct number of significant figures. mL Note: Reference the Phase change properties of pure substances table for additional information. kJ -H₂O mol
When 29.5 mL of 0.500 M H2SO4 is added to 29.5 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g · ° C.)
When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)
The temperature of 127.4 g of water rises from 18.6 °C to 30.9 °C when 0.1000 mol of H+ is reacted with 0.1000 mol of OH-. If the specific heat capacity of water is 4.184J/g°C, calculate qwater.
In a coffee cup calorimeter, a student places 0.350 g of magnesium, followed by addition of 45.0 mL of 1.00 M hydrochloric acid. After the reaction took place, a the temperature rose from 21.5oC to 54.2oC. If the reaction solution has the same properties of water and the calorimeter constant is 5.38 J oC-1, how much heat was released from the reaction and what is the enthalpy of the reaction in kJ mol-1? Answer choices for heat released from reaction: -7.89 kJ, -4.12 kJ, -6.50 kJ, -5.66 kJ
A quantity of 8.90 × 102 mL of 0.800 M HNO3 is mixed with 8.90 × 102 mL of 0.400 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO3 reacts with 0.500 mol Ba(OH)2 is -56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water (1.00 g/mL and 4.184 J/g °C, respectively). What is the final temperature of the solution?
A sample of NaOH (MM = 40.00 g/mol) with a mass of 1.811 g was added to a solution of HNO3 in a coffee cup calorimeter for a final volume of 100.0 mL. If both solutions were initially at 24.5 °C and the temperature of the resulting solution was recorded as 27.0 °C, determine the AH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH. Assume that the density and the heat capacity of the resulting solution are the same as water, 1.00 g/mL and 4.184 J/(g x °C) respectively. Your Answer: Answer units
When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.10 mL of 3.00 M HCI, both initially at room temperature (22.00 °C), the temperature increased to 29.60 °C. The resultant salt solution had a mass of 28.10 g and a specific heat capacity of 3.74 J K- g-. What is the heat capacity of the calorimeter (in J/°C)?Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ mol-1
A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC

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