Atomic weights in g/mole: H = 1.0, C = 12.0, N = 14.0, O = 16.0, F = 19.0, Cl = 35.5, Cu = 63.5 = 8.314 J/mole K 411.0 g diethyl ether exists as an ideal gas at T 80 °C. 1) The gas is cooled to 35 °C, the boiling point. The gas is condensed, and the resulting liquid is cooled to 0 °C. What is AS for this process? (Cp of liquid = 172.5 J/mole K, AHvap = 27.1 kJ/mole)

Atomic weights in g/mole: H = 1.0, C = 12.0, N = 14.0, O = 16.0, F = 19.0, Cl = 35.5, Cu = 63.5 = 8.314 J/mole K 411.0 g diethyl ether exists as an ideal gas at T 80 °C. 1) The gas is cooled to 35 °C, the boiling point. The gas is condensed, and the resulting liquid is cooled to 0 °C. What is AS for this process? (Cp of liquid = 172.5 J/mole K, AHvap = 27.1 kJ/mole)

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

A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.
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.)
An enthalpy of solution discusses the enthalpy change of dissolving an ionic compound in water. 8.31 grams of NaOH is added to 152.5 mL of H2O at 298 K. What is the final temperature of this solution after the salt dissolves if the enthalpy of solution for NaOH is -44.5 kJ/mol? The heat capacity of water is 4.184 J/ (g K) and the density of water is 1.00 g/mL.
Suppose that 125 mL of 0.1125 M HCI is reacted with 155 mL of 0.1010 M NaOH in a coffee-cup calorimeter. HCl(aq) + NaOH H20(1) + NaCl(aq) -56 KJ mol ΔΗ If the initial temperature of the mixture is 22.1°C, calculate the final temperature of the mixture given the following information. Ssolution = 4.1 g.°C %3D Dsolution = 1.02 mL 25.5 °C 24.3 °C 22.8 °C O 19.8 °C
2. Please calculate the standard enthalpy of reaction (AHrxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na2O(s) → 2NaNO2 (s) NO(g) + NO₂(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O2(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ = 507.31 kJ/mol AH = -427.14 kJ/mol AH = - 42.68 kJ/mol 34.35 kJ/mol ΔΗ ΔΗ = 44.012 kJ/mol =
What is the enthalpy of reaction, ΔHrxn for the reaction of nitrogen gas with oxygen gas to produce NO2(g), based on the following information? These reactions are not at standard state or at 298 K. N2(g) + O2(g) → 2 NO(g); ΔH = 332.9 kJ2 NO2(g) → 2 NO(g) + O2(g); ΔH = 718.4 kJ Report your answer in kJ to 1 decimal place.
A 0.50 Kg Cu container holds 1.00 kg of water at 20° C. A 0.10 kg iron ball at 120° C is dropped into the water. What is the final equilibrium temperature of the mixture? C of copper = 0.093 cal/ g C°; c of iron = 0.115 cal/g Co C ofwater = 1 cal/ g Co
What is the enthalpy change when 8.20 moles ammonium chloride form in the following equation? N2 (g) + 4 H2 (g) + Cl2 (g) --> 2 NH4Cl (s) Delta H = – 628.8 kJ a. – 2.58 x 103 kJ b. – 1.29 x 103 kJ c. + 314.4 kJ d. – 314.4 kJ e. – 628.8 kJ f. – 5.16 x 103 kJ g. none of these d. – 314.4 kJ
27. When 0.0500 mol of CH4 (g) burns, 40.1 kJ of heat is produced. What is the change in enthalpy (AH) in kJ for the following reaction: CH4 (g) (a) +802 kJ/mol + 202 (g) (b) -802 kJ/mol , CO₂ (g) + 2H₂O(g) + Heat (c) +40.1 kJ/mol (d) -40.1 kJ/mol
When a 6.00 g6.00 g sample of KClKCl is dissolved in water in a calorimeter that has a total heat capacity of 4.47 kJ⋅K−1,4.47 kJ⋅K−1, the temperature decreases by 0.310 K.0.310 K. Calculate the molar heat of solution of KCl.
using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1. (A) 0.397 J·g–1·°C–1. (B) 0.447 J·g–1·°C–1. (C) 1.28 J·g–1·°C–1. (D) 1.55 J·g–1·°C–1.