Answer the following question 1) Dry nitrogen gas (100.0L) was bubbled through liquid chloroform, CHCI 3, at agiven temperature and the evaporated chloroformcondensed; its mass was then measured. Using the databelow, calculate the heat of vaporization (kJ/mol) ofchloroform?Temperature, Â°C Mass CHCl3 collected, g12.19 72.0527.03 131.72) Calculate the pOH after addition of 15.97 mL of 0.1762M LIOH to 25.00 mL of 0.1582 M HBr.3) Calculate the pOH after addition of 15.85 mL of 0.1209M KOH to 25.00 mL of 0.1798 M CH 3CH 2CH ₂CO 2H. Ka(CH 3CH 2CH 2CO₂H) = 1.500e-54)Calculate the pH after addition of 24.38 mL of 0.1148 MHCIO 4 to 25.00 mL of 0.1989 M CH 3CH 2NH 2. K b(CH3CH 2NH2) = 6.400e-4.5) What is the solubility of Sb 2S 3 if it's K sp is 1.700e-93?

“Since you have posted multiple questions, we will provide the solution only to the first question…

Answer the following question 1) Dry nitrogen gas (100.0 L) was bubbled through liquid chloroform, CHCI 3, at a given temperature and the evaporated chloroform condensed; its mass was then measured. Using the data below, calculate the heat of vaporization (kJ/mol) of chloroform? Temperature, Â°C Mass CHCl3 collected, g 12.19 72.05 27.03 131.7

Answer the following question 1) Dry nitrogen gas (100.0 L) was bubbled through liquid chloroform, CHCI 3, at a given temperature and the evaporated chloroform condensed; its mass was then measured. Using the data below, calculate the heat of vaporization (kJ/mol) of chloroform? Temperature, Â°C Mass CHCl3 collected, g 12.19 72.05 27.03 131.7

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

Hydrogen is considered a "green fuel" and can be used in fuel cells. One method of hydrogen production is shown below and is known as steam methane reforming: CH₂(g) + H₂O(g) 3 H₂(g) + CO(g) Calculate the volume in KL, at SATP, of H₂(g) produced when 903 g of CH4(9) reacts with excess steam. Do not show your work in the space provided. Record only your final answer with the correct number of significant digits and the proper units. Answer:
Calculate the total enthalpy change (kJ) for the following reaction: H2O (s, 90 g, –10. oC) --> H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 kJ/mol.)
17. Use the enthalpies of formation and the enthalpy of reaction given below to determine the 16. Use enthalpies of formation given to determine the standard enthalpy of reaction or following: 00 2 Al (s) + Fe2O3 (s) Al2O3 (s) +2 Fe AH° =??? AH° (kJ/mol) -825.5 -1676 enthalpy of formation for solid CaC2. CaC2 (s) + 2 H2O (1)→ Ca(OH)2 (s) + C2H2 (g) AH° =-127 kJ AH°r (kJ/mol) ??? -286 -986 +227 11 The haat of vanorization of a liquid (AHvan) is the heat required to vaporize 1.00 g of a Linto o
The following information is given for benzene, CáHá, at 1atm: AHvap(80.1 °C) = 30.7 kJ/mol boiling point 80.1 °C specific heat liquid = KJ 1.74 J/g °C At a pressure of 1 atm, what is AH in kJ for the process of condensing a 47.4 g sample of gaseous benzene at its normal boiling point of 80.1 °C.
Write a balanced thermochemical equation with phase labels for the Haber process with the heat energy as part of the equation.
1a. Calculate the pressure of a sample of 1 mole of argon gas in a 0.1500 L flask at -10.2 ℃ using the ideal gas law and the Van der Waals equation. The a value for argon is 1.34 (L 2 ∙ atm/mol2 ) and the b value is 0.0322 (L/mol). Show all work Ideal pressure= ? real pressure =? 1b.Why is there a difference in the real gas pressure and the ideal pressure? Explain what assumption(s) of the kinetic molecular theory of gases break down under these conditions.
9. Use the AH°f and AH°rxn information provided to calculate AH°f for IF. Provide the formation reactions that gave rise to the AHºf values. Why is the AHºf value for 12(g) zero? IF7(g) + 12(s)→ IFs(g) + 2 IF(g) AH°rxn = -89 kJ AH (kJ/mol) IF7(g) -941 IFs(g) -840
A 23.0 gram sample of an alloy was heated to 100.00 °C and dropped into a beaker containing 92 grams of water at 25.84 °C. The temperature of the water rose to a final temperature of 27.84 °C. Neglecting heat losses to the room and the heat capacity of the beaker itself, what is the specific heat of the alloy in /g°C? а. 2.16 ОБ. 0.464 O c. 0.232 O d. 4.32
Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO2) into solid calcium oxide and gaseous carbon dioxide. C 2. Suppose 86.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 260.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.