Using the table provided, calculate the thermodynamic property of interest for each given reaction. Thermodynamic Data at 25 °C Species AHe in kJ/mol AGº in kJ/mol So in J/(mol·K) Cu (s) 33.2 Cu (g) 337.4 297.7 166.4 CuO (s) -157.3 -129.7 42.6 H2 (g) 131.0 H2O (g) -241.8 -228.6 188.7 H2O (€) -285.8 -237.2 69.9 NO (g) 91.3 87.6 210.8 NO2 (g) 33.2 51.3 240.1 N¿O4 (E) -19.5 97.5 209.2 N2O4 (g) 9.16 99.8 304.4 O2 (g) 205.0 O Determine AS° for H2 (g) + ½ O2 (g) → H2O (g) at 25 °C. (11) Determine AG° for 2 Cu (s) + O2 (g) → 2 CuO (s) at 25 °C. (1i1) Determine AH° for H2O (€) → H2O (g) at 100 °C.

Using the table provided, calculate the thermodynamic property of interest for each given reaction. Thermodynamic Data at 25 °C Species AHe in kJ/mol AGº in kJ/mol So in J/(mol·K) Cu (s) 33.2 Cu (g) 337.4 297.7 166.4 CuO (s) -157.3 -129.7 42.6 H2 (g) 131.0 H2O (g) -241.8 -228.6 188.7 H2O (€) -285.8 -237.2 69.9 NO (g) 91.3 87.6 210.8 NO2 (g) 33.2 51.3 240.1 N¿O4 (E) -19.5 97.5 209.2 N2O4 (g) 9.16 99.8 304.4 O2 (g) 205.0 O Determine AS° for H2 (g) + ½ O2 (g) → H2O (g) at 25 °C. (11) Determine AG° for 2 Cu (s) + O2 (g) → 2 CuO (s) at 25 °C. (1i1) Determine AH° for H2O (€) → H2O (g) at 100 °C.

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

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.)
Determine the heat involved in the combustion of liquid hydrazine by using the following reactions. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ) ΔH°= –1013 kJ/molN2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –317 kJ/mol2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –142.9 kJ/molH2(g) + ½ O2(g) → H2O(ℓ) ΔH°= –285.8 kJ/mol Then, Launching a small spacecraft to study Jupiter required approximately 28 million kJ. Assume that hydrazine was the only fuel. What mass of hydrazine, in kilograms, was needed for the launch?
Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction. If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?
A student dissolves 11.0 g of ammonium chloride (NH, CI) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 20.0 °C to 16.8 °C over the course of 6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH,CI(s) NH (aq) + Cl (aq) db You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ…
A student dissolves 11.8 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 20.0 °C to 33.6 °C over the course of 8 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na (aq) + OH (ag) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NaOH. O…
Given the following equation, N20(g) + NO28) → 3 NO(g) AG°rxn = -23.0 kJ Calculate AG° rxn for the following reaction. 3N20(g) + 3NO2(g) 9 NO(g) -23.0 kJ 69.0 kJ -69.0 kJ -7.67 kJ 23.0 kJ
A student dissolves 12.3 g of ammonium chloride (NH4C1) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 21.0 °C to 17.4 °C over the course of 3.6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) NH(aq) + Cl(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 2 significant digits. → Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothe nic, endothermic or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ per mole of NH Cl. rxn exothermic 0…
The standard enthalpy of formation of SnCl₂ (s) is - 340 kJ/mol and that for SnCl4 (s) is-511 kJ/mol. From these data, we can calculate that for the reaction SnCl₂ (s) + Cl₂ (g) →→SnCl4 (s), the value of AH O cannot be determined as AH, for Cl₂ (g) is not given. O equals - 851 kJ. O equals + 171 kJ. O equals - 171 kJ.
3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.
In a coffee cup calorimeter with a heat capacity of 21.5 J/ºC, 225 mL of 0.20 M KOH at 22.3 ºC neutralizes 225 mL of 0.20 M HCl at 22.3 ºC. After the reaction occurs, the temperature of the resulting mixture is 29.2 ºC. The density of the final solution is 1.00 g/mL and the specific heat is 4.18 J/g°C. Calculate the Heat of neutralization of KOH.
Calcium ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) Ca (s) 0 0 41.4 Ca (g) 178.2 144.3 158.9 Ca2+ (g) 1925.9 CaC2 (s) -59.8 -64.9 70.0 CaCO3 (s, calcite) -1206.9 -1128.8 92.9 CaCl2 (s) -795.8 -748.1 104.6 CaF2 (s) -1219.6 -1167.3 68.9 CaH2 (s) -186.2 -147.2 42.0 CaO (s) -635.1 -604.0 39.8 CaS (s) -482.4 -477.4 56.5 Ca(OH)2 (s) -986.1 -898.5 83.4 Ca(OH)2 (aq) -1002.8 -868.1 -74.5 Ca3(PO4)2 (s) -4126.0 -3890.0 241.0 CaSO4 (s) -1434.1 -1321.8 106.7 CaSiO3 (s) -1630.0 -1550.0 84.0 Carbon ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) C (s, graphite) 0 0 5.7 C (s, diamond) 1.9 2.9 2.4 C (g) 716.7 671.3 158.1 CCl4 (l) -135.4 -65.2 216.4 CCl4 (g) -102.9 -60.6 309.9 CHCl3 (l) -134.5 -73.7 201.7 CHCl3 (g) -103.1 -70.3 295.7 CH4 (g) -74.8 -50.7 186.3 CH3OH (g)…
Consider the reaction. 2 Fe₂0₂4Fe +30₂ AHin = +824.2 kJ The formation of 62.0 g of Fe results in the release of 229 kJ of heat. the absorption of 229 kJ of heat. O the release of 12800 kJ of heat. the release of 915 kJ of heat. the absorption of 12800 kJ of heat. the absorption of 915 kJ of heat.