3. Use the information contained in "Lab Exercise 11.B" on page 506 in the textbook toanswer the following questions.a. Use the reaction equations and reaction enthalpies shown in the introduction section tocalculate the following:CSH12CL)-> 5C(s) -6H2009) 6420 LLA• a reaction enthalpy for the combustion of pentane• a molar enthalpy of combustion for pentane[ 3488.7 kJ and 3488.7 kJ/mol ]Answer:CsHizW180₂(g)-56₂9³ +64₂0(1)CSH12C1-35CCs) +6 H₂(g)H₂Ocg)-4₂0x66H20c9-620(1) @4=90.65*5cc)+502) -560₂ (9)*6=64₂ (9)+302(g)-(20(g0Answer:b. Use the calorimetric data provided to calculate a molar enthalpy of combustion forpentane56cs)+50₂(g) - 500₂6g6H₂(g) +30₂9-6H₂0lgAnswer:-3488.7hJI mol[3.35 x10 kJ/mol ]=-mclt= -mcat/n=C1.24 kg (4.197( 37.6-18.4)(0.0297907718mol)-3.35×103 kJ/mol[3.98 % ]-=-3488.7 Kc. Calculate the percentage error between the value calculated in question 3.a(theoretical value) and the value calculated in question 3.b (experimental value).04. Use the information contained in "Lab Exercise 11.D" on page 513 in the textbook toanswer the following questions.

Part (c)Theoretical Value = 3488.7 kJ/mol (Obtained in 3a)Experimental Value = 3.35 x…

Answered: - Calculate the percentage error…

- Calculate the percentage error between the value calculated in question 3.a (theoretical value) and the value calculated in question 3.b (experimental value). [3.98 % ]

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...

See similar textbooks

Similar questions

10. CHALLENGE. You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at standard pressure and temperature): 1 volume "gas X" + 2 volumes "gas Y" → 2 volumes compound I 2 volumes "gas X" + 1 volume "gas Y" → 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y and suggest identities.
The label on a bottle of medicine reads "Each 5 mL teaspoonful contains glucose, 1.87 g; levulose, 1.87 g; and phosphoric acid, 21.2mg." a. Find the amount of phosphoric acid in the recommended dosage of two teaspoons. b. If the bottle contains 3 ounces, find the quantity of phosphoric acid in the bottle. ( 1 oz ≈ 30 mL; 1 tsp ≈ 5 mL)
Part A.Calculate the percent carbon in fructose, C6H12O6 Express your answer are using to decimal places Part B. Calculate the percent hydrogen and fructose, C6H12O6
Commercial ibuprofen tablets contain 200 mg of ibuprofen each. The commercial tablets have the active ingredient (ibuprofen) in addition to several other additives (e.g. starch, sucrose, etc) to assist in digestion. There are 6 tablets that are used in the experiment. The maximum amount of available ibuprofen is (6 x 200 mg) = 1200 mg. Six pills Pure Ibup (after m.p. recrys.) Crude ibup. Gross mass (g) 2.89 29.50 2.09 Tare mass (g) 0.89 28.32 1.00 Net mass (g) |2g 1.18 g 1.09 g 70-71C 1) Calculate the percentage of ibuprofen in each pill. 2) Calculate the percent recovery of ibuprofen from the pills, based on the crude ibuprofen mass. 3) Calculate the percent recovery of pure ibuprofen from the crude. 4) Why does the melting point (70-71)above match neither the enantiomers' nor the racemate's? Does it mean that the substance is impure, or perhaps isn't even ibuprofen at all? (Racemic mixture:75-77C, Enantiomer:52-53C)
What is the percent by weight (w/w%) of sugar in soda? Assume the average mass of sugar in soda is 22.0 g and the total mass is 370.0 g.
Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you. You determined experimentally the density of a solution in triplicate. Considering the results what is the %RSD of results? Answer your question with the correct number of significant figures. Please enter answer as a % not in decimal form. Trial 1: 1.014 g/mL Trial 2: 0.914 g/mL Trial 3: 1.190 g/mL
Please answer question number 2 correctly with the correct answer. there is a picture of an example of a ''Dimensional analysis Format' below. please write out all work showing the math in dimensional analysis format. (please show all work) Question 8: Calculate the mass in grams of each of the following: C.) 0.00100 mol silicon tetrahydride (SiH4) D. ) 1.50 x 10^-2 mol molecular oxygen (O2) E. 2.30 mol ethylene glycol (C2H6O2)
What is the mass, in grams, of each of the following? I.) 2.1×10−3 mol Sb Express your answer using two significant figures. II.) 3.59×10−2 mol Ba Express your answer using three significant figures. III.) 44.2 mol Xe Express your answer using three significant figures. IV.) 1.1 mol W Express your answer using two significant figures.
X, Mass of sample (g) = 0.7 Y, Mass of benzoic acid (g) = 0.3 Z, Mass of pellet (g) = 0.9 calculate the follwing below information Mass of sample in pellet = Mass of benzoic acid in pellet =
The compound PClx contains 85.14% chlorine by mass. What is the value of x? Enter your response as a whole number.
Calculate the number of grams of CaCO3 present and convert to mg. (enter your answer with 3 significant figures)
7. How many moles are contained in each of the following? A. 21.0 gg CaCa Express your answer using three significant figures. B. 5.30 gg SS Express your answer using three significant figures. C. 40.0 gg H2OH2O Express your answer using three significant figures.