Explanation Method used: Newton’s Method: 1. Pick an initial estimate x 0 of the root c. 2. Find a new estimate using the iterative formula x n + 1 = x n − f ( x n ) f ′ ( x n ) , n = 0 , 1 , 2 , … 3. Compute | x n − x n + 1 | . If the number is less than a prescribed positive number, then stop the iteration. The required approximation to the root x = c is x = x n + 1 . Calculation: The pair of functions is given by f ( x ) = 2 − x 2 and g ( x ) = ln x . Use online graphing calculator, graph the pair of functions f ( x ) = 2 − x 2 and g ( x ) = ln x as shown below in Figure 1. From Figure 1, it is observed that the point of intersection of these graphs is ( 1.314 , 0.273 ) . To refine the approximation of the x -coordinate of the point of intersection, equate the two functions f ( x ) = 2 − x 2 and g ( x ) = ln x . 2 − x 2 = ln x 2 − x 2 − ln x = 0 h ( x ) = 2 − x 2 − ln x Find the derivative of h ( x ) = 2 − x 2 − ln x as follows. h ′ ( x ) = − 2 x − 1 x The required iterative formula is, x n + 1 = x n − 2 − x n 2 − ln x n − 2 x n − 1 x n = − 2 x n 2

APPLIED CALCULUS FOR MGRL, LIFE, SOC SCI

10th Edition

ISBN: 9780357465400

Author: Tan

Publisher: CENGAGE L

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Chapter 11.7, Problem 28E

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To make: A rough sketch of the pair of the graphs of f(x)=2−x2 and g(x)=lnx to approximate the points of intersection of the two graphs, and then apply Newton’s method to refine the approximation of the x-coordinate of the point of intersection.

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Chapter 11.7, Problem 27E

Chapter 11.7, Problem 29E

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Question 3: A sealed flask at room temperature contains a mixture of neon (Ne) and nitrogen (N2) gases. Ne has a mass of 3.25 g and exerts a pressure of 48.2 torr. . N2 contributes a pressure of 142 torr. • What is the mass of the N2 in the flask? • Atomic mass of Ne = 20.1797 g/mol • Atomic mass of N = 14.0067 g/mol Solution: We will use the Ideal Gas Law to determine the number of moles of each gas and calculate the mass of N2. PV = nRT where: • P = total pressure • V volume of the flask (same for both gases) n = number of moles of gas • R 0.0821 L atm/mol K • T = Room temperature (assume 298 K) Since both gases are in the same flask, their partial pressures correspond to their mole fractions. Step 1: Convert Pressures to Atmospheres 48.2 PNe = 0.0634 atm 760 142 PN2 = = 0.1868 atm 760 Step 2: Determine Moles of Ne nNe = mass molar mass 3.25 nNe 20.1797 nne 0.1611 mol Step 3: Use Partial Pressure Ratio to Find n

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Chapter 11 Solutions

APPLIED CALCULUS FOR MGRL, LIFE, SOC SCI

Ch. 11.1 - Prob. 1CQ Ch. 11.1 - Prob. 2CQ Ch. 11.1 - Prob. 1E Ch. 11.1 - In Exercises 110, find the first three Taylor...Ch. 11.1 - Prob. 3E Ch. 11.1 - Prob. 4E Ch. 11.1 - Prob. 5E Ch. 11.1 - Prob. 6E Ch. 11.1 - Prob. 7E Ch. 11.1 - Prob. 8E

Ch. 11.1 - In Exercises 110, find the first three Taylor...Ch. 11.1 - Prob. 10E Ch. 11.1 - Prob. 11E Ch. 11.1 - Prob. 12E Ch. 11.1 - Prob. 13E Ch. 11.1 - Prob. 14E Ch. 11.1 - In Exercises 1120, find the nth Taylor polynomial...Ch. 11.1 - Prob. 16E Ch. 11.1 - Prob. 17E Ch. 11.1 - Prob. 18E Ch. 11.1 - Prob. 19E Ch. 11.1 - Prob. 20E Ch. 11.1 - Prob. 21E Ch. 11.1 - Prob. 22E Ch. 11.1 - Prob. 23E Ch. 11.1 - Prob. 24E Ch. 11.1 - Prob. 25E Ch. 11.1 - Prob. 26E Ch. 11.1 - Prob. 27E Ch. 11.1 - Prob. 28E Ch. 11.1 - Prob. 29E Ch. 11.1 - Prob. 30E Ch. 11.1 - Prob. 31E Ch. 11.1 - Prob. 32E Ch. 11.1 - Prob. 33E Ch. 11.1 - Prob. 34E Ch. 11.1 - Let f(x) = ex. a. 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To make: A rough sketch of the pair of the graphs of f ( x ) = 2 − x 2 and g ( x ) = ln x to approximate the points of intersection of the two graphs, and then apply Newton’s method to refine the approximation of the x -coordinate of the point of intersection.

Solution Summary: The author illustrates Newton's method of calculating the x-coordinate of the points of intersection of two graphs using an online graphing calculator.

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To make: A rough sketch of the pair of the graphs of f(x)=2−x2 and g(x)=lnx to approximate the points of intersection of the two graphs, and then apply Newton’s method to refine the approximation of the x-coordinate of the point of intersection.

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Chapter 11 Solutions