lution of HI was found to have a pOH of 13.35 at 25 °C. What is the concentration of HI? a. 0.52 M b. 1.13 M c.0.22 M D d.0.43 M Oe.1.6 x 10-6 M A change in a system occurs such that 51.3 J of work is done on the surroundings and 45.9 J of heat flows in to the system. What is the chang energy of the system? O a. 45.9 J O b. -51.3 J Oc. -5.4J O d. 97.2 J O e.5.4J

lution of HI was found to have a pOH of 13.35 at 25 °C. What is the concentration of HI? a. 0.52 M b. 1.13 M c.0.22 M D d.0.43 M Oe.1.6 x 10-6 M A change in a system occurs such that 51.3 J of work is done on the surroundings and 45.9 J of heat flows in to the system. What is the chang energy of the system? O a. 45.9 J O b. -51.3 J Oc. -5.4J O d. 97.2 J O e.5.4J

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

Why did you use 4.184 J/goC as the specific heat capacities of the solutions? a. Because all kinds of solution have a constanst specific heat capacity of 4.184 J/goC. b. Because it was assumed that the solutions are concentrated. c. Because it was assumed that the solutions are dilute. d. Because this specific heat capacity is constant for solutions performed in any constant-pressure calorimeter.
Which of the following reaction sequences would be best for converting para-bromoanisole to ortho-ethylanisole? a. (i) Mg in ether (ii) C2H5CI / AlCl3 b. (i) Mg in ether (ii) aqueous acid (iii) C2H5CI / AlCl3 c. (i) C2H5Cl/AlCl3 (ii) Mg in ether (iii) aqueous acid d. (i) H2 / Pt catalyst (ii) C2H5CI / AlCl3
A system absorbs 423 J of heat while doing 241 J of work. What is the value of AU ? Lütfen birini seçin: O a. +182 J O b. -182 J O C. +664 J O d. -664 J O e. -364 J
A system does 435 kJ of work(w) and loses 312 kJ of heat(q) to the surroundings. What is the change in internal energy of the system? O a. -747KJ Ob. 740KJ. c. -465kJ O d. 465KJ
Which of the following statement is/are true about the first law of thermodynamics? I. Energy is can be transferred and transformed. II. Energy lost by a system is equal to the energy gained by the surroundings. III. The sum of the energy of the system and the surroundings is always greater than 0. O II only O Il and III only O l and III only O I, Il and II O I only O Il only O l and Il only
14. Which of the following statements are true about a system that absorbs 300J of heat from the surroundings while performing 150 J of work on the surroundings? I. The internal energy change of the system is +150 J. The process described above is exothermic. The internal energy change of the system is -150 J. The process described above is endothermic. II. III. IV. а. I, II b. II, III с. I, IV d. III, IV
100 g of hot metal was put in 222.2 g of water in a container. Both the container and the water are at 20 deg C. Cp of water is 4.184 J K−1 g −1 and Cp of metal is 0.4444 J K−1 g −1. 2.222 kJ K−1 is the heat capacity of the container. 22 C is the final temperature of the metal, water and the container. Determine the initial temperature of the metal.
O THERMOCHEMISTRY Understanding the definition of enthalpy ARL 0/5 Measurements show that the energy of a mixture of gaseous reactants increases by 252. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 117. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic
a. Determine whether energy as heat is evolved or required in the following process at constant pressure: N₂O4 (g) decomposes to form NO2 (g). Energy is required. O Energy is evolved. b. Determine whether work was done on the system or the system does work on the surroundings in the following process at constant pressure: N₂O4 (g) decomposes to form NO2 (g). O Work was done on the system. No work is done. O The system does work on the surroundings. c. Determine whether energy as heat is evolved or required in the burning of ethyne at constant pressure: 2 C₂ H₂ (g) + 5 O2 (g) → 4 CO2 (g) + 2 H₂O(g) Energy is required. O Energy is evolved. d. Determine whether work was done on the system or whether the system does work on the surroundings in the burning of ethyne at constant pressure: 2 C₂ H₂(g) + 5 O2 (g) → 4 CO2 (g) + 2 H₂O(g) Work was done on the system. O No work is done. O The system does work on the surroundings.
The figure shows a closed cycle for a gas (the figure is not drawn to scale). The change in the internal energy of the gas as it moves from a to c along the path abc is -200 J. As it moves from c to d, 180 J must be transferred to it as heat. An additional transfer of 80 J to it as heat is needed as it moves from d to a. Analyze the figure using first law of thermodynamics and determine the work done on the gas as it moves from c to d?
What is the change in internal energy for a system if the system absorbs 322 kJ of heat and has 750.0 kJ of work done on the system? Select one: a. 1.07 x 10^3 kJ b. –1.07 x 10^3 kJ c. 536 kJ d. 1072 kJ e. –536 kJ f. none of these g. 428 kJ h. –428 kJ i. –1072 kJ
In an experiment, 1.0 mol each of H2(g) and I2(g) are placed in an empty 5.0-L flask and the flask is then sealed. These gases react as follows. H2 (9) + I,(9) 2 HI(g) Which of the following statement is/are true? (i) The value of Kincreases as the system approaches equilibrium. (ii) The value of K decreases as the system approaches equilibrium. (iii) The total pressure increases as the system approaches equilibrium. (i) and (iii) are true (ii) and (iii) are true only (iii) is true none of these are true all of these are true