In an experiment mixing Ammonium nitrate of 5.00g mass and water with 200g of mass incalorimeter. The initial temperature is 20.0 Celsius and final temperature is 18.13 Celsius. Findthe q water, q dissolution, mass of solid NH4NO3, moles of NH4NO3 and the change in enthalpy(delta H) of NH4NO3 dissolution.

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Answered: In an experiment mixing Ammonium…

Chemistry

10th Edition

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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If 100.0 g H2O at 20.1 °C is mixed with 100.0 g H2O at 98.4 °C, what is the final temperature of the solution mixture ? Assume no heat is lost to the vessel in which the mixing takes place. Use CH2O = 1.00 cal/g×°C
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5.21 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
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2.948 g of NH4Cl (53.19 g/mol) are added to 50.0 mL of water (18.02 g/mol, density = 1.00 g/mL) and the temperature changes from 22.30oC to 18.90oC. Use this information to calculate the enthalpy change (kJ/mol) for the reaction illustrated in equation 6 of the laboratory procedure. Use 4.18 J/(goC) as the specific heat of the solution.
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2.857 g of NH4Cl (53.19 g/mol) are added to 50.0 mL of water (18.02 g/mol, density = 1.00 g/mL) and the temperature changes from 22.30oC to 18.90oC. Use this information to calculate the enthalpy change (kJ/mol) for the reaction illustrated in equation 6 of the laboratory procedure. Use 4.18 J/(goC) as the specific heat of the solution. The equation is NH4Cl (s) --> NH4Cl (aq)
2.887 g of NH4Cl (53.19 g/mol) are added to 50.0 mL of water (18.02 g/mol, density = 1.00 g/mL) and the temperature changes from 22.30oC to 18.90oC. Use this information to calculate the enthalpy change (kJ/mol) for the reaction illustrated in equation 6 of the laboratory procedure. Use 4.18 J/(goC) as the specific heat of the solution. (6) NH4Cl(s) → NH4Cl(aq) ∆H6 (measured) Your answer should have 3 sig figs
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?
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