5. 83 kJ of heat are exchanged between the system and surroundings in an endothermic reaction,...
A system which does work on the surroundings with no heat change (i.e., q = 0) has: Ow=AU Ow=-AU w>0, AU < 0 O w<0, AU > 0 Ο w > Δυ Question 2 4 pts For the reaction: 2A + B2 -> 2AB AH = +50.0 kJ. The reaction is endothermic The bond energy for each A-B bond is 50.0 kJ The molecule AB contains less energy than A or B2 Heat is released to the surroundings
QUESTION 7 When heat is not exchanged between a system and its surroundings (q = 0), which one of the following terms is used to describe the process? O A. adiabatic B. isothermal C. isochoric OD. isobaric E. endothermic QUESTION 8 A photon possesses an energy of 1.35 x 10-18 Joules of energy. What is the wavelength of this photo in nanometers (nm)? Remember: E= hv&vBot;and C = v, where c= 3.00 x 100 meters/second.
5. For a particular process, q=-17 kJ and w = 21 kJ. Which of the following statements is false? a. Heat flows from the system to the surroundings. b. The system does work on the surroundings. c. AE = +4 kJ d. The process is exothermic. e. None of the above is false.
on 4 of 15 A system does 501 kJ of work and loses 286 kJ of heat to the surroundings What is the change in internal energy, AE, of the system? Note that internal energy is symbolized as AU in some sources. AE = kJ
1. A gas absorbs 0.0 J of heat and then performs 30.8 J of work. The change in internal energy of the gas is a. 61.6 J. b. 30.8 J. c. -61.6 J. d.-30.8 J. e. none of these 2. Which of the following statements correctly describes the signs of q and w for the following exothermic process at P= 1 atm and T = 370 K? H2O(g) → H2O(1) a. q and w are negative. b. is positive, wis...
Part A A chemical system produces 135 kJ of heat and does 29 kJ of work. What is AE for the surroundings? C 160 kJ C-160 kJ C -110 kJ C110 kJ Request Answer Submit
A system releases 661 kJ of heat and does 100 kJ of work on the surroundings. What is the change in internal energy of the system?
At 25°C, the following heats of reaction are known: AH (kJ/mol 167.4 2CIF + 02 →Cl20 + F20 2ClF3 + 202 →Cl20+3F20 341.4 2F2 + 02 → 2F20 At the same temperature, calculate ΔH for the reaction: ClF + F2 → CIF3 -43.4 A. -217.5 kJ/mol B.-130.2 kJ/mol C. +217.5 kJ/mol ○ D.-108.7 kJ/mol E. none of these QUESTION 4 Consider the reaction: When a 12.9-g sample of ethyl alcohol(molar mass 46.07 g/mol) is burned, how much energy is released...
1.) A system absorbs 1.56E+2 kJ of heat and the surroundings do 1.107E+2 kJ of work on the system. What is the change in internal energy (in kJ) (ΔU) of the system? 2.) A sample of gas in a cylinder is provided with 6.221E+2 kJ of heat. This causes a piston to then compresses the gas by doing 4.343E+2 kJ of work to the gas. What is the change in internal energy of the gas during this compression? 3.)A gas...
A system does 531 kJ of work and loses 241 kJ of heat to the surroundings. What is the change in internal energy, Δ E , of the system? Note that internal energy is symbolized as Δ U in some sources.