28. The volume of four moles of an ideal monatomic gas at 600 °K is halved while the pressure is tripled. What is the change (in kilojoules, kJ) of the internal energy of the gas? (a) 14.96 (b) 22.66 (c) 15.00 (d) 31.06 (e) none of these god) ene 200 1s 2sy bumotanom A en 001.0.21 51mploy saod 01 x 0.1 to slquior sa.E 24.8 EP 2

28. The volume of four moles of an ideal monatomic gas at 600 °K is halved while the pressure is tripled. What is the change (in kilojoules, kJ) of the internal energy of the gas? (a) 14.96 (b) 22.66 (c) 15.00 (d) 31.06 (e) none of these god) ene 200 1s 2sy bumotanom A en 001.0.21 51mploy saod 01 x 0.1 to slquior sa.E 24.8 EP 2

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...

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10,11) pt pt of t [References] Use the References to access important values if needed for this question. The following thermochemical equation is for the reaction of hydrogen sulfide (g) with water(1) to form hydrogen (g) and sulfur dioxide(g). ΔΗ 207 kJ H₂S(g) + 2H₂O(g) 3H₂(g) + SO2(g) When 10.6 grams of hydrogen sulfide (g) react with excess water(1), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
10.) The heat of formation of H2SO4 (ag) is -909.27 kl/mol. Which of the following is the thermochemical equation for the formation of aqueous sulfuric acid? А.) SO3 (g) + H20 (I) - → H2SO4 (aq) + 909.27 kJ B.) SO2 (g) + ½ 02 (g) + H20 (1) → H2SO4 (aq) + 909.27 kJ C.) H2 (g) + S (s) + 2 02 (g) → H2SO4 (aq) + 909.27 kJ D.) SO2 (g) + H2O2 (aq) → H2SO4 (aq) + 909.27 kJ
The complete combustion of ethanol, C2H5OH1l2, to formH2O1g2 and CO21g2 at constant pressure releases 1235 kJ ofheat per mole of C2H5OH. (a) Write a balanced thermochemicalequation for this reaction. (b) Draw an enthalpy diagramfor the reaction.
In the figure below, the change in internal energy of a gas that is taken from A to C along the blue path is +900 J. The work done on the gas along the red path ABC is -590 J. S D C V (a) How much energy must be added to the system by heat as it goes from A through B to C? J (b) If the pressure at point A is five times that of point C, what is the work done on the system in going from C to D? J (c) What is the energy exchanged with the surroundings by heat as the gas goes from C to A along the green path? נן (d) If the change in internal energy in going from point D to point A is +580 J, how much energy must be added to the system by heat as it goes from point C to point D? J
The oxidation of the sugar glucose, C6H12O6, is described by the following equation: C6 H12 O6(s) + 6O2(g) ⟶ 6CO2(g) + 6H2 O(l) ΔH = −2816 kJThe metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body. a) How much heat in kilojoules can be produced by the metabolism of 1.0 g of glucose? (b) How many Calories can be produced by the metabolism of 1.0 g of glucose?
A 148 g sample of an unknown metal at 74.0 oC is placed in a beaker containing 80.0 g of H2O at 25 oC. The final temperature of the metal sample and water is 32 oC. cH2O(l) = 4.184 j/ g oC SHOW ALL WORK (a) What is the specific heat (c) of the metal? (b) 5 common metals have the following specific heat capacities (c) [given in units of J/g oC] : Aluminum: 0.921 Copper: 0.377 Gold: 0.126 Iron: 0.461 Nickel: 0.502 Your sample is most likely to be which metal?
When 745 J of energy in the form of heat is transferred from the environment to a gas, the expansion of the gas does 312 J of work on theenvironment. What is the change in internalenergy of the gas?
ulate het reaction enthalpy O O D Dwayne V Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) - CH,OH(1) + H,O(1) AH =-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH,OCH,(g) + H,0(1) AH - 8. kJ olb Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. Explanation Check O 2021 McGraw Hill LLC. All Rights Reserved. Terms of UseI Privacy Center Accessibility 4:25 AM ENG 12/14/2021 35°F Clear O Type here to search
The complete combustion of ethanol, C2H5OH(l), to formH2O(g) and CO2(g) at constant pressure releases 1235 kJ ofheat per mole of C2H5OH. (a) Write a balanced thermochemicalequation for this reaction. (b) Draw an enthalpy diagramfor the reaction.
iv to vi please
Measurements show that the energy of a mixture of gaseous reactants increases by 316. 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 -171. 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. 09 O exothermic Is the reaction exothermic or endothermic? O endothermic X G C
The overall reaction in a commercial heat pack can be repre- sented as 4Fe(s) + 30₂(g) 2Fe₂O3(s) AH = -1652 kJ d. How much heat is released when 10.0 g Fe and 2.00 g O₂ are reacted?