Iron (Fe)2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of thesolution went up to 50.1°C.99.725a. Is this dissolution reaction exothermic? esWhy?The ran reultd in heet increeseH0.of theti= 23.7%っ』Cb. Calculate quH,0, using Equation 1.CmesAt5486.769= 5486.70Jjoulesc.Find AH for the reaction as it occurred in the calorimeter (Eq. 5).9emcst-6036.3joulesΔΗ=*49.72 Hho (E4= 6636.25ご G036.33A#ニ-4 ,9=Gのムこ(continued on following page)- (G0363))= -G036.3AF 106Experiment 14 Heat Effects and Calorimetryd.Find AH for the dissolution of 1.00 g NaOH in water.AH = - qmcatAH =kJ/ge. Find AH for the dissolution of 1 mole NaOH in water.AH =kJ/molf.Given that NaOH exists as Na* and OH ions in solution, write the equation for the reaction thatoccurs when NaOH is dissolved in water.Given the following heats of formation, AH, in kJ per mole, as obtained from a table of AH, data,g.calculate AH for the reaction in Part (f). Compare your answer with the result you obtained in Part (e).NAOH(s), -425.6; Na*(aq), -240.1; OH (aq), -230.0ΔΗ=kJ/mol

When 4.98 g of NaOH was dissolved in 49.72 g of water ., ∆Hrxn = - 6036.3 Joule

d. Find AH for the dissolution of 1.00 g NAOH in water. AH=-qmcst AH = kJ/g e. Find AH for the dissolution of 1 mole NaOH in water. AH = kJ/mol %3D f. Given that NaOH exists as Na* and OH ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water. g. Given the following heats of formation, AH, in kJ per mole, as obtained from a table of AH data, calculate AH for the reaction in Part (f). Compare your answer with the result you obtained in Part (e). NAOH(s), -425.6; Na*(aq), -240.1; OH (aq), -230.0 ΔΗ- kJ/mol

d. Find AH for the dissolution of 1.00 g NAOH in water. AH=-qmcst AH = kJ/g e. Find AH for the dissolution of 1 mole NaOH in water. AH = kJ/mol %3D f. Given that NaOH exists as Na* and OH ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water. g. Given the following heats of formation, AH, in kJ per mole, as obtained from a table of AH data, calculate AH for the reaction in Part (f). Compare your answer with the result you obtained in Part (e). NAOH(s), -425.6; Na*(aq), -240.1; OH (aq), -230.0 ΔΗ- kJ/mol

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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Using the thermodynamic tables find the enthalpy of reaction for the reaction B2H6 (g) + 6 F2 (g) --> 2 BF3 (g) + 6 HF (g) a. – 3877 kJ b. – 3912 kJ c. + 3877 kJ d. + 3947 kJ e. – 3947 kJ f. none of these g. + 572 kJ
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The addition of 1.170 g of zinc metal to 0.03580 mol HCl in a total of 0.100Lin a coffee-cup calorimeter causes the temperature to increase from 15.00°C to 21.51°C. What is the value of AHrxn for the following reaction? Zn(s) +2HC1(aq) → → ZnCl, (aq) +H,(g)
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Question 15.62
6. Use the standard heat of formation AHf to calculate the AH for the reaction: a. C3H8 (g) + 5 O2 (g) C3H8 -104KJ O₂ =0 KI 3 CO2 (g) + 4H₂O (1) CO2 -393.5 KJ H₂O -286 KJ
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3.02 g of sodium sulfate was mixed into a solution containing 48.5 mL of 0.185 mol/L aqueous silver nitrate: Calculate the maximum mass (in g) of precipitate that can form. Note: Balanced chemical eq. with state of each compound required. 2. What is the molar concentration of sodium ions in the resulting solution?
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