For problems 1 through 3 below, the initial state of 1 mole of an ideal gas is P₁ = 3 atm, V₁ = 1 liter, and U₁ = 456 J, and its final state is P2 = 2 atm, V₂ = 3 liters, and U₂ = 912 J. 1. The gas is allowed to expand at constant pressure to a volume of 3 liters. It is then cooled at constant volume until its pressure is 2 atm. a) Show this process on a PV diagram, and calculate the work done by the gas. b) Find the heat added during this process.

For problems 1 through 3 below, the initial state of 1 mole of an ideal gas is P₁ = 3 atm, V₁ = 1 liter, and U₁ = 456 J, and its final state is P2 = 2 atm, V₂ = 3 liters, and U₂ = 912 J. 1. The gas is allowed to expand at constant pressure to a volume of 3 liters. It is then cooled at constant volume until its pressure is 2 atm. a) Show this process on a PV diagram, and calculate the work done by the gas. b) Find the heat added during this process.

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 gaseous reaction occurs at a constant pressure of 40.4 bar and releases 58.6 kJ of heat. Before the reaction, the volume of the system was 9.00 L. After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change, AU, in kilojoules. Express your answer with the appropriate units.
Given the following equations, find the AHºf of one mol of HCI from its elements. Show the balanced chemical equation for the formation of HCl from H2 and Cl2. Target Equation: A) N2 (g) + 3 H2 (g) → 2 NH3 (g) AH°rxn = -91.8 kJ B) N2 (g) + 4 H2 (g) + Cl2 (g) → 2 NHẠCI (s) AH°, rxn = -628.8 kJ C) NH3 (g) + HCI (g) → NHẠCI (s) AH°rxn = -176.2 kJ
A gas expands against a variable opposing pressure given by P = 10/V atm, where V is the volume of the gas at each stage of expansion. Further, in expanding from 10 to 100 liters, the gas undergoes a change in internal energy of AE = 100 cal. How much heat, in calories, is absorbed by the gas during the process? [NOTE: 1 atm = 24.22 cal] %3D
What is the value of Kc at 1000.0°C?
thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J'g.°C', is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The aluminum sample starts off at 92.4 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 23.2 °C. The pressure remains constant at 1 atm. insulated container water sample Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. a calorimeter Submit Assignment Continue 62021 McGraw Hill LLC. Al Rights Reserved. Terms of UseI Privacy Center Accessibility
1 A 25.0 g sample of quartz, which has a specific heat capacity of 0.730 JgC, is dropped into an insulated container containing 300.0 g of water at 75.0 °C and a constant pressure of 1 atm. The initial temperature of the quartz is 4.1 °C. Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. C 0 x10 X S
Nitric acid, HNO3, reacts with potassium hydroxide as follows: HNO3(aq) + KOH(aq) ⟹ KNO3(aq) + H2O(l) A student places 55.0mL of 1.3M HNO3 in a coffee cup calorimeter, and noted that the temperature was 23.5oC. 55mL of 1.3M KOH also at 23.5oC was added. After quickly stirring with a thermometer, the temperature rose to 31.8oC. Calculate the heat generated by the reaction.
+2 -3 a. solid calcium nitride plus heat Ca Na 3 Ca +2N b. solid lead (IV) carbonate plus heat рысозда 1→→ Pb 0₂ + 2003 c. solid chromium (III) sulfate hexahydrate plus heat d. sodium metal plus nitrogen gas
A 56.2 g sample of aluminum, which has a specific heat capacity of 0.897 J-g¹C¹, is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the aluminum sample. Be sure your answer is rounded to the correct number of significant digits. °C X Ś thermometer- insulated. container water sample a calorimeter
The gas cyclopropane, C3H6(g), can be used in welding. When cyclopropane is burned in oxygen, the reaction is: 2 C3H6(g) + 9 O₂(g)6 CO₂(g) + 6 H₂O(g) (a) Using the following data, calculate AH° for this reaction. AH kJ mol-¹: C3H6(g) = 53.3; CO₂(g) = -393.5; H₂O(g) = -241.8 4 AH° = kj (b) Calculate the total heat capacity of 6 mol of CO₂(g) and 6 mol of H₂O(g), using CcO₂(g) = 37.1 J K-1 mol-¹ and CH₂O(g) = 33.6 J K-¹ mol-¹. C = JK-1 (c) When this reaction is carried out in an open flame, almost all the heat produced in part (a) goes to raise the temperature of the products. Assuming that the reactants are at 25°C, calculate the maximum flame temperature that is attainable in an open flame burning cyclopropane in oxygen. The actual flame temperature would be lower than this because heat is lost to the surroundings. Maximum temperature °℃
Use Hess's law to Calculate the AH of the reaction C₂H₂(g) + H₂(g) → C₂H,(g) from the following data. Identify the "manipulation" for each reaction C₂H₂(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(1) C₂H₂(g) + 3% O₂(g) 2 CO₂(g) + 3 H₂O(1) H₂(g) + O₂(g) → H₂O(1) ΔΗ = -1411 kJ AH = -1560 kJ AH = -285.8 kJ
Thermodynamics 3. A 2000 mL container holds 0.100 mol of He (g) at 300 °C. Treat He(g) as an ideal gas for the following problems. Report energies in units of Joules. Increasing Volume n₁ = 0.1 mol V₁ = 2000 mL T₁ = 300° C P₁ = n = 0.1 mol V = 1000 mL T₂ = A P₂= P₁ = C B n = 0.1 mol V = 2000 mL T3 = P3 = 2.5 x P₁ = D n = 0.1 mol V = 1000 mL T₁ = P4 = P3= Increasing Pressure a. Calculate all the missing values in the following diagram. Report pressures in units of atm and temperatures in units of degrees Celsius.