Heat of Reaction, Mole Fraction1. A group of students perform a series ofexperiments mixing HCI with an unknown baseof the formula M(OH)n. For each trial the totalvolume of acid and base was 50.0 mL. Theconcentration of the acid and base solutionswere 0.6000 M. The data is plotted in the graphprovided. The density of the aqueous solutionis assumed to be 1.00 g/mL and the specificheat of water is 4.18 J/g °Cin joules160014001200100080060040020000.00000.6000 M HCI0 20000.6000 M(OH)x0 40000 6000Mole Fraction of Acid0 800010000a) What is the limiting reagent at a mole fraction of 0.6 of acid?b) Write a balanced equation for the reaction of M(OH), with HCI. (You must determine "n")c) For one trial, the students measured a temperature change of + 2.9 °C. Calculate q.d) The students calculated a value of q of 1.5 x 10³ J for one of their trials. For this trial0.015 mol of HCI and 0.015 mol of M(OH), were used. Calculate heat per mole for thisreaction.

Given: Volume of solution = 50.0 mL density of solution = 1.0 g/mL specific heat of solution = 4.18…

A group of students perform a series of experiments mixing HCI with an unknown base of the formula M(OH)n. For each trial the total volume of acid and base was 50.0 mL. The concentration of the acid and base solutions were 0.6000 M. The data is plotted in the graph provided. The density of the aqueous solution is assumed to be 1.00 g/mL and the specific heat of water is 4.18 J/g °C To 1600 1400 1200 1000 800 600 400 200 0 0 0000 0.6000 M HCl vs. 0.6000 M(OH), 0 2000 04000 06000 Mole Fraction of Acid 0 8000 10000 a) What is the limiting reagent at a mole fraction of 0.6 of acid? b) Write a balanced equation for the reaction of M(OH), with HCI. (You must determine "n") c) For one trial, the students measured a temperature change of + 2.9 °C. Calculate q. The students calculated a value of q of 1.5 x 103 J for one of their trials. For this trial 0.015 mol of HCI and 0.015 mol of M(OH), were used. Calculate heat per mole for this reaction.

A group of students perform a series of experiments mixing HCI with an unknown base of the formula M(OH)n. For each trial the total volume of acid and base was 50.0 mL. The concentration of the acid and base solutions were 0.6000 M. The data is plotted in the graph provided. The density of the aqueous solution is assumed to be 1.00 g/mL and the specific heat of water is 4.18 J/g °C To 1600 1400 1200 1000 800 600 400 200 0 0 0000 0.6000 M HCl vs. 0.6000 M(OH), 0 2000 04000 06000 Mole Fraction of Acid 0 8000 10000 a) What is the limiting reagent at a mole fraction of 0.6 of acid? b) Write a balanced equation for the reaction of M(OH), with HCI. (You must determine "n") c) For one trial, the students measured a temperature change of + 2.9 °C. Calculate q. The students calculated a value of q of 1.5 x 103 J for one of their trials. For this trial 0.015 mol of HCI and 0.015 mol of M(OH), were used. Calculate heat per mole for this reaction.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.9QE

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