When a 4.25-g sample of solid sodium nitrate dissolves in 50.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 24.00°C to 28.90°C. What is AH (in kJ/mol NaNO3) for the dissolution of sodium nitrate: NaNO3(s) → Na*(aq) + NO3 "(aq) Assume that the specific heat of the solution is the same as that of pure water (4.18 J/g-K). O1.17 kJ/mol O 20.5 kJ/mol 4.90 kJ/mol O 1.02 kJ/mol Submit Request Answer

When a 4.25-g sample of solid sodium nitrate dissolves in 50.0 g of water in a coffee-cup calorimeter (Figure 5.18), the temperature rises from 24.00°C to 28.90°C. What is AH (in kJ/mol NaNO3) for the dissolution of sodium nitrate: NaNO3(s) → Na*(aq) + NO3 "(aq) Assume that the specific heat of the solution is the same as that of pure water (4.18 J/g-K). O1.17 kJ/mol O 20.5 kJ/mol 4.90 kJ/mol O 1.02 kJ/mol Submit Request Answer

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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When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X- (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
11. A 114.06 mL sample of 0.245 M aqueous hydrochloric acid is added to 122.18 mL of 0.172 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 498.075 J/K. The following reaction occurs when the two solutions are mixed. HCl(aq) + NH3(aq) → NH4Cl(aq) The temperature increase is 2.03°C. Calculate ΔH rxn. Answer=____________________kJ/mol
66.667 ml of 3.000 M H2SO4 (aq) solution was neutralized by the stoichiometric amount of 4.000 M Al(OH)3 solution in a coffee cup calorimeter. The initial temperature of the solutions was 22.3 ºC and after mixing the temperature raised to 24.7 ºC. If the heat capacity of coffee cup is 1.10 J/g ºC, calculate the DHreaction in J/mol Al2(SO4)3.
In a coffee cup calorimeter, 50.0 mL of 0.139 M AgNO3 and 50.0 mL of 0.139 M HI are mixed. The following reaction occurs. Ag+ (aq) + I (aq) → Agi(s) If the two solutions are initially at 21.74°C, and if the final temperature is 23.60°C, calculate AH for the reaction in kJ/mol of AgI formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors. Supplemental Data
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5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the temperature of the solution increases by 1.60oC. Calculate ΔH for the reaction in kJ/mol of KOH .The specific heat capacity of the solution is 4.18 J/goC ( Hint: the mass of the solution is 105g) (Hint #2: is this + or -?) Your answer should be in kJ/mol and have 3 sig figs
2 A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.34 g of CoSO4(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 26.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
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 =
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