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Chemistry |! Straighterline |! Comprehensive |!
Exam |! with |! verified |! answers
An |! endothermic |! reaction |! causes |! the |! surroundings |! to: A. |! warm |! up B. |! become |! acidic C. |! condense D. |! decrease |! in |! temperature E. |! release |! CO2 |! - |! Correct |! answer |! ✔D An |! exothermic |! reaction |! causes |! the |! surroundings |! to: A. |! warm |! up B. |! become |! acidic C. |! expand D. |! decrease |! its |! temperature E. |! release |! CO2 |! - |! Correct |! answer |! ✔A Copper |! metal |! has |! a |! specific |! heat |! of |! 0.385 |! J/g•oC |! and |! has |! a |! melting |! point |! of |! 1083oC. |! calculate |! the |! amount |! of |! heat |! required |! to |! raise |! the |! temperature |! of |! 22.8 |! g |! of |! Cu |! from |! 20.0oC |! to |! 875oC. A. |! 1.97 |! 10 |! ─ |! 5 |! J |!
B. |! 1.0 |! 10 |! ─ |! 2 |! J
C. |! 329 |! J
D. |! 7.51 |! kJ E. |! 10.5 |! kJ |! - |! Correct |! answer |! ✔D Calculate |! the |! amount |! of |! heat |! necessary |! to |! raise |! the |! temperature |! of |! 12.0 |! kg |! of |! water |! from |! 15.4oC |! to |! 93.0oC. A. |! 0.027 |! kJ |! B. |! 324 |! kJ |! C. |! 389 |! kJ |! D. |! 931 |! kJ |! E. |! 3890 |! kJ |! - |! Correct |! answer |! ✔E How |! much |! heat |! is |! required |! to |! raise |! the |! temperature |! of |! 1500 |! g |! of |! water |! from |! 25oC |! |! to |! 52oC? A. |! 1500 |! kJ |! B. |! 169 |! kJ |! C. |! 6.27 |! kJ |! D. |! 40.5 |! J |! E. |! 40.5 |! kJ |! - |! Correct |! answer |! ✔B How |! many |! degrees |! of |! temperature |! rise |! will |! occur |! when |! a |! 25.0 |! g |! block |! of |! aluminum |! absorbs |! 10 |! kJ |! of |! heat? |! The |! specific |! heat |! of |! Al |! is |! 0.900 |! J/g•oC. A. |! 0.44oC |! B. |! 22.5oC |! C. |! 225oC |! D. |! 360oC |! E. |! 444oC |! - |! Correct |! answer |! ✔E If |! 325 |! g |! of |! water |! at |! 4.2oC |! absorbs |! 12.28 |! kJ, |! then |! what |! is |! the |! final |! temperature |! of |! the |! water? A. |! 4.21oC |! B. |! 4.8oC |! C. |! 9.0oC |! D. |! 13.2oC |! E. |! 2938oC |! - |! Correct |! answer |! ✔D
D. |! 1.34 |! kJ/oC E. |! 752.1 |! kJ/oC |! - |! Correct |! answer |! ✔D Naphthalene |! combustion |! can |! be |! used |! to |! determine |! the |! heat |! capacity |! of |! a |! bomb |! calorimeter. |! The |! heat |! of |! combustion |! of |! naphthalene |! is |! 40.1 |! kJ/g. |! When |! 0.8210 |! g |! of |! naphthalene |! was |! combusted |! in |! a |! calorimeter |! containing |! 1000 |! g |! of |! water |! a |! temperature |! rise |! of |! 4.21oC |! was |! observed. |! What |! is |! the |! heat |! capacity |! of |! the |! bomb |! calorimeter |! excluding |! the |! water? A. |! 32.9 |! kJ/oC B. |! 7.8 |! kJ/oC C. |! 1.76 |! kJ/oC D. |! 1.76 |! kJ/oC E. |! 15.3 |! kJ/oC |! - |! Correct |! answer |! ✔C Which |! of |! the |! following |! processes |! is |! endothermic? a. |! O2(g) |! + |! 2H2(g) |! 2H2O(g) |! b. |! H2O(g) |! H2O(l) c. |! 3O2(g) |! + |! 2CH3OH(g) |! 2CO2(g) |! + |! 2H2O(g) |! d. |! H2O(s) |! H2O(l) |! - |! Correct |! answer |! ✔D A |! 100 |! mL |! sample |! of |! 0.200 |! M |! aqueous |! hydrochloric |! acid |! is |! added |! to |! 100 |! mL |! of |! 0.200 |! M |! aqueous |! ammonia |! in |! a |! calorimeter |! whose |! heat |! capacity |! is |! 480 |! J |! K |! ─ |! 1. |! The |! following |! reaction |! occurs |! when |! the |! two |! solutions |! are |! mixed. |! HCl(aq) |! + |! NH3(aq) |! NH4Cl(aq)
The |! temperature |! increase |! is |! 2.34oC. |! Calculate |! ΔH |! per |! mole |! of |! HCl |! neutralized. |! A. |! 154 |! kJ |! B. |! 44.5 |! kJ |! C. |! 22.5 |! kJ |! D. |! ─22.5 |! kJ |! E. |! ─56.2 |! kJ |! - |! Correct |! answer |! ✔E A |! 0.1326 |! g |! sample |! of |! magnesium |! was |! burned |! in |! an |! oxygen |! bomb |! calorimeter. |! The |! Htotal |! heat |! capacity |! of |! the |! calorimeter |! plus |! water |! was |! 5760 |! J/oC. |! If |! the |! temperature |! rise |! of |! the |! calorimeter |! with |! water |! was |! 0.570oC, |! calculate |! the |! enthalpy |! of |! combustion |! of |! magnesium. Mg(s) |! + |! 1/2O2(g) |! MgO(s) |! A. |! ─3280 |! kJ/mol |! B. |! ─24.8 |! kJ/mol |! C. |! 435 |! kJ/mol |! D. |! 106 |! kJ/mol |! E. |! ─602 |! kJ/mol |! - |! Correct |! answer |! ✔E Which |! one |! of |! the |! following |! reactions |! occurring |! at |! 25oC |! does |! the |! symbol |! ΔHof[H2SO4(l)] |! refer |! to? A. |! 2H(g) |! + |! S(g) |! + |! 4O(g) |! H2SO4(l) B. |! H2(g) |! + |! S(g) |! + |! 2O2(g) |! H2SO4(l) C. |! H2SO4(l) |! H2(g) |! + |! S(s) |! + |! 2O2(g) D. |! H2SO4(l) |! 2H(g) |! + |! S(s) |! + |! 4O(g) E. |! H2(g) |! + |! S(s) |! + |! 2O2(g) |! H2SO4(l) |! - |! Correct |! answer |! ✔E Which |! one |! of |! the |! following |! reactions |! occurring |! at |! 25oC |! does |! the |! symbol |! ΔHof[HNO3(l)] |! refer |! to? A. |! H(g) |! + |! N(g) |! + |! O3(g) |! HNO3(l) B. |! 1/2H2(g) |! + |! 1/2N2(g) |! + |! 3/2O2(g) |! HNO3(l)
Find |! the |! standard |! enthalpy |! of |! formation |! of |! ethylene, |! C2H4(g), |! given |! the |! following |! data: C2H4(g) |! + |! 3O2(g) |! 2CO2(g) |! + |! 2H2O(l) |! ΔHof |! = |! ─1411 |! kJ C(s) |! + |! O2(g) |! CO2(g) |! ΔHof |! = |! ─393.5 |! kJ H2(g) |! + |! 1/2O2(g) |! H2O(l) |! ΔHof |! = |! ─285.8 |! kJ A. |! 52 |! kJ B. |! 87 |! kJ C. |! 731 |! kJ D. |! 1.41 |! 103 |! kJ E. |! 2.77 |! 103 |! kJ |! - |! Correct |! answer |! ✔A Octane |! (C8H18) |! undergoes |! combustion |! according |! to |! the |! following |! thermochemical |! equation: 2C8H18(l) |! + |! 25O2(g) |! 16CO2(g) |! + |! 18H2O(l) |! ΔHorxn |! = |! ─11,020 |! kJ. Given |! that: |! ΔHof[CO2(g)] |! = |! ─393.5 |! kJ/mol ΔHof[H2O(l)] |! = |! ─285.8 |! kJ/mol Calculate |! the |! enthalpy |! of |! formation |! of |! 1 |! mole |! of |! octane. A. |! ─210 |! kJ |! B. |! ─11,230 |! kJ |! C. |! 22,040 |! kJ |! D. |! ─420 |! kJ |! E. |! 420 |! kJ |! - |! Correct |! answer |! ✔A Glycine |! C2H5O2N |! is |! important |! for |! biological |! energy. |! The |! combustion |! of |! glycine |! is |! given |! by |! the |! equation, 4C2H5O2N(s) |! + |! 9O2(g) |! 8CO2(g) |! + |! 10H2O(l) |! + |! 2N2(g) |! ΔHorxn |! = |! ─3857 |! kJ
Given |! that |! ΔHof[CO2(g)] |! = |! ─393.5 |! kJ/mol, |! and |! ΔHof[H2O(l)] |! = |! ─285.8 |! kJ/mol. |! Calculate |! the |! enthalpy |! of |! formation |! ΔHof |! per |! mole |! of |! glycine. A. |! ─537.2 |! kJ/mol B. |! ─268.2 |! kJ/mol |! C. |! 2149 |! kJ/mol D. |! ─3178 |! kJ/mol E. |! ─964 |! kJ/mol |! - |! Correct |! answer |! ✔A Calculate |! ΔHorxn |! for |! the |! following |! reaction. 2H2O2(l) |! 2H2O(l) |! + |! O2(g) |! Use |! the |! following |! information: |! ΔHof |! (H2O2(l)) |! = |! -187.6 |! kJ/mol |! ; |! ΔHof |! (H2O(l)) |! = |! -285.8 |! kJ/mol |! ; |! ΔHof |! (O2(g)) |! = |! 0 |! kJ/mol A. |! 53.0 |! kJ |! B. |! 98.2 |! kJ |! C. |! -98.2 |! kJ |! D. |! 196.4 |! kJ |! E. |! ─196.4 |! kJ |! - |! Correct |! answer |! ✔E Given |! 2Al(s) |! + |! 3/2O2(g) |! Al2O3(s) |! ΔHof |! = |! ─1670 |! kJ |! What |! is |! ΔH |! for |! the |! reaction? 2Al2O3(s) |! 4Al(s) |! + |! 3O2(g) |! ΔHorxn |! = |!? A. |! 3340 |! kJ |! B. |! 1670 |! kJ |! C. |! ─3340 |! kJ |! D. |! ─1670 |! kJ |! E. |! ─835 |! kJ |! - |! Correct |! answer |! ✔A Calculate |! the |! enthalpy |! change |! for |! the |! reaction: |! C(graph) |! + |! 2H2(g) |! + |! 1/2O2(g) |! CH3OH(l)
2SO2 |! + |! O2 |! 2SO3 |! ΔHorxn |! = |! ─198 |! kJ. What |! is |! the |! enthalpy |! change |! (ΔHo) |! for |! the |! decomposition |! of |! one |! mole |! of |! SO3? A. |! 198 |! kJ |! B. |! ─99 |! kJ |! C. |! 99 |! kJ |! D. |! 396 |! kJ |! E. |! ─198 |! kJ |! - |! Correct |! answer |! ✔C Given: |! H2(g) |! + |! 1/2O2(g) |! H2O(l) |! ΔHof |! = |! ─286 |! kJ |! What |! is |! the |! enthalpy |! change |! for |! the |! following |! reaction? 2H2O(l) |! 2H2(g) |! + |! O2(g) |! ΔHorxn |! = |!? A. |! ΔHo |! = |! ─286 |! kJ |! B. |! ΔHo |! = |! +286 |! kJ C. |! ΔHo |! = |! ─572 |! kJ D. |! ΔHo |! = |! +572 |! kJ E. |! ΔHo |! = |! ─143 |! kJ |! - |! Correct |! answer |! ✔D A |! home |! aquarium |! is |! an |! example |! of |! an |! open |! system |! - |! Correct |! answer |! ✔TRUE In |! an |! endothermic |! process |! heat |! is |! absorbed |! by |! the |! system. |! - |! Correct |! answer |! ✔TRUE The |! heat |! absorbed |! by |! a |! system |! at |! constant |! pressure |! is |! equal |! to |! ΔE |! + |! PΔV. |! - |! Correct |! answer |! ✔TRUE
The |! work |! done |! on |! the |! surroundings |! by |! the |! expansion |! of |! a |! gas |! is |! w |! = |! ─PΔV. |! - |! Correct |! answer |! ✔TRUE The |! heat |! capacity |! of |! 20.0 |! g |! of |! water |! is |! 83.7 |! J/oC. |! - |! Correct |! answer |! ✔TRUE If |! 2Mg(s) |! + |! O2(g) |! 2MgO(s) |! ΔHo |! = |! ─1203.6 |! kJ; |! then |! for |! Mg(s) |! + |! 1/2O2(g) |! MgO(s) |! the |! enthalpy |! change |! is |! ΔHf |! = |! ─601.8 |! kJ |! - |! Correct |! answer |! ✔TRUE Chemical |! reactions |! in |! a |! bomb |! calorimeter |! occur |! at |! constant |! pressure Conditions. |! - |! Correct |! answer |! ✔FALSE The |! specific |! heats |! of |! water |! and |! iron |! are |! 4.184 |! and |! 0.444 |! J/g•oC, |! respectively. |! When |! equal |! masses |! of |! water |! and |! iron |! both |! absorb |! the |! same |! amount |! of |! heat, |! the |! temperature |! increase |! of |! the |! water |! will |! be |! 5.42 |! times |! greater |! than |! that |! of |! the |! iron. |! - |! Correct |! answer |! ✔FALSE Pentaborane |! B5H9(s) |! burns |! vigorously |! in |! O2 |! to |! give |! B2O3(s) |! and |! H2O(l). |! Write |! and |! balance |! the |! combustion |! equation. |! Calculate |! the |! ΔHorxn |! for |! the |! combustion |! of |! 1 |! mol |! of |! B5H9 |! given |! the |! following |! enthalpies |! of |! formation. |! ΔHof[B2O3(s)] |! = |! ─1273.5 |! kJ/mol ΔHof[B5H9(s)] |! = |! 73.2 |! kJ/mol
The |! combustion |! of |! butane |! produces |! heat |! according |! to |! the |! equation: |! 2C4H10(g) |! + |! 13O2(g) |! 8CO2(g) |! + |! 10H2O(l) |! ΔHorxn= |! ─5314 |! kJ |! How |! many |! grams |! of |! butane |! must |! be |! burned |! to |! release |! 6375 |! kJ |! of |! heat? |! A. |! 1.20 |! g |! B. |! 139 |! g |! C. |! 0.0413 |! g |! D. |! 69.7 |! g |! E. |! 97.8 |! g |! - |! Correct |! answer |! ✔B Given |! the |! following |! information: CaO(s) |! + |! H2O(l) |! Ca(OH)2(s) |! ΔHorxn |! = |! ─64.8 |! kJ/mol How |! many |! grams |! of |! CaO |! must |! react |! in |! order |! to |! liberate |! 525 |! kJ |! of |! heat? A. |! 6.92 |! g |! B. |! 56.1 |! g |! C. |! 455 |! g |! D. |! 606 |! g |! E. |! 3.40 |! 104 |! g |! - |! Correct |! answer |! ✔C The |! combustion |! of |! pentane |! produces |! heat |! according |! to |! the |! equation: C5H12(l) |! + |! 8O2(g) |! 5CO2(g) |! + |! 6H2O(l) |! ΔHorxn= |! ─3510 |! kJ |! How |! many |! grams |! of |! CO2 |! are |! produced |! per |! 2500 |! kJ |! of |! heat |! released? |! A. |! 0.0809 |! g |! B. |! 3.56 |! g |! C. |! 31.3 |! g |! D. |! 157 |! g |! E. |! 309 |! g |! - |! Correct |! answer |! ✔D The |! combustion |! of |! butane |! produces |! heat |! according |! to |! the |! equation: 2C4H10(g) |! + |! 13O2(g) |! 8CO2(g) |! + |! 10H2O(l) |! ΔHorxn= |! ─5314 |! kJ |! How |! many |! grams |! of |! CO2 |! are |! produced |! per |! 1.00 |! 104 |! kJ |! of |! heat? A. |! 23.4 |! g |! B. |! 44.0 |! g |! C. |! 82.3 |! g |! D. |! 187 |! g |! E. |! 662 |! g |! - |! Correct |! answer |! ✔E An |! average |! home |! in |! Colorado |! requires |! 20 |! GJ |! of |! heat |! per |! month. |! How |! many |! grams |! of |! natural |! gas |! as |! methane |! must |! be |! burned |! to |! supply |! this |! energy? |! CH4(g) |! + |! 2O2(g) |! CO2(g) |! + |! 2H2O(l) |! ΔHorxn= |! ─890.4 |! kJ |!
A. |! 1.4 |! 103 |! g |! B. |! 3.6 |! 105 |! g |! C. |! 7.1 |! 10-4 |! g |! D. |! 2.2 |! 104 |! g |! E. |! 1.4 |! 104 |! g |! - |! Correct |! answer |! ✔B Given |! the |! thermochemical |! equation: 2SO2(g) |! + |! O2(g) |! 2SO3(g) |! ΔHorxn= |! ─198 |! kJ How |! much |! heat |! is |! evolved |! when |! 600 |! g |! of |! SO2 |! is |! burned? A. |! 5.46 |! 10 |! ─ |! 2 |! kJ B. |! 928 |! kJ C. |! 1.85 |! 103 |! kJ D. |! 59,400 |! kJ E. |! 3.71 |! 103 |! kJ |! - |! Correct |! answer |! ✔B How |! much |! heat |! is |! given |! off |! to |! the |! surroundings |! when |! 9.0 |! g |! of |! aluminum |! react |! |! according |! to |! the |! equation? 2Al |! + |! Fe2O3 |! Al2O3 |! + |! 2Fe |! ΔHorxn= |! ─849 |! kJ A. |! 7.6 |! 103 |! kJ B. |! 2.8 |! 102 |! kJ C. |! 1.4 |! 102 |! kJ D. |! 5.6 |! 102 |! kJ E. |! 2.5 |! 103 |! kJ |! - |! Correct |! answer |! ✔C How |! much |! heat |! is |! absorbed |! from |! the |! surroundings |! when |! 15 |! g |! of |! O2 |! react |! according
A. |! 1.97 |! kJ |! B. |! 8.26 |! kJ |! C. |! 508 |! kJ |! D. |! 547 |! kJ |! E. |! 555 |! kJ |! - |! Correct |! answer |! ✔B According |! to |! the |! first |! law |! of |! thermodynamics: A. |! Energy |! is |! neither |! lost |! nor |! gained |! in |! any |! energy |! transformations. B. |! Perpetual |! motion |! is |! possible. C. |! Energy |! in |! a |! closed |! system |! is |! conserved. D. |! Energy |! is |! being |! created |! as |! time |! passes. |! We |! have |! more |! energy |! in |! the |! universe |! now |! than |! when |! time |! began. |! - |! Correct |! answer |! ✔C 10.1 |! g |! CaO |! is |! dropped |! into |! a |! styrofoam |! coffee |! cup |! containing |! 157 |! g |! H2O |! at |! 18.0oC. |! |! If |! the |! following |! reaction |! occurs, |! then |! what |! temperature |! will |! the |! water |! reach |! assuming |! that |! the |! cup |! is |! a |! perfect |! insulator |! and |! that |! the |! cup |! absorbs |! only |! a |! negligible |! amount |! of |! heat? |! CaO(s) |! + |! H2O(l) |! Ca(OH)2(s) |! ΔHorxn |! = |! ─64.8 |! kJ/mol A. |! 18.02oC |! B. |! 35.8oC |! C. |! 311oC |! D. |! 42.2oC |! E. |! 117oC |! - |! Correct |! answer |! ✔B Calculate |! the |! work |! done |! in |! joules |! when |! 2.5 |! mol |! of |! H2O |! vaporizes |! at |! 1.0 |! atm |! and |! |! 25oC. |! Assume |! the |! volume |! of |! liquid |! H2O |! is |! negligible |! compared |! to |! that |! of |! vapor. |! Given |! 1 |! L•atm |! = |! 101.3 |! J. A. |! 6190 |! kJ |! B. |! 6.19 |! kJ |! C. |! 61.1 |! J |! D. |! 5.66 |! kJ |! E. |! 518 |! J |! - |! Correct |! answer |! ✔B
A |! gas |! is |! compressed |! in |! a |! cylinder |! by |! a |! constant |! pressure |! of |! 10 |! atm |! from |! a |! volume |! H |! of |! 20 |! L |! to |! 2.0 |! L. |! Calculate |! the |! work |! done |! on |! the |! system. A. |! 1.01 |! 104 |! J |! B. |! -180 |! J |! C. |! 1.81 |! 104 |! J |! D. |! ─1.81 |! 104 |! J |! E. |! 180 |! J |! - |! Correct |! answer |! ✔C Calculate |! the |! work |! done |! against |! an |! atmospheric |! pressure |! of |! 1.00 |! atm |! when |! 500.0 |! g |! of |! zinc |! dissolves |! in |! excess |! acid |! at |! 30.0oC. Zn(s) |! + |! 2H+(aq) |! Zn2+(aq) |! + |! H2(g) |! A. |! w |! = |! +22.4 |! kJ B. |! w |! = |! +24.9 |! kJ C. |! w |! = |! 0 D. |! w |! = |! ─2.52 |! kJ E. |! w |! = |! ─19.3 |! kJ |! - |! Correct |! answer |! ✔E A |! gas |! is |! allowed |! to |! expand |! at |! constant |! temperature |! from |! a |! volume |! of |! 1.0 |! L |! to |! 10.1 |! L |! against |! an |! external |! pressure |! of |! 0.50 |! atm. |! If |! the |! gas |! absorbs |! 250 |! J |! of |! heat |! from |! the |! surroundings, |! what |! are |! the |! values |! of |! q, |! w, |! and |! ΔE? |! q |! w |! ΔE |! A. |! 250 |! J |! ─460 |! J |! ─210 |! J B. |! ─250 |! J |! ─460 |! J |! ─710 |! J C. |! 250 |! J |! 460 |! J |! 710 |! J D. |! ─250 |! J |! 460 |! J |! 210 |! J
Calculate |! the |! ΔH° |! value |! for |! the |! reaction |! C3H4(g) |! + |! 2 |! H2(g) |! C3H8(g) |! A. |! ─292 |! kJ/mol B. |! +292 |! kJ/mol C. |! +850 |! kJ/mol ─850 |! kJ/mol |! - |! Correct |! answer |! ✔A Calculate |! the |! ΔH° |! of |! the |! following |! reaction: C2H4(g) |! + |! H2(g) |! C2H6(l) |! Given |! the |! standard |! enthalpies |! of |! formation |! of |! the |! following |! species: |! Substance |! ΔH°f |! --------------------------------- |! C2H4(g) |! +52.3 |! kJ |! C2H6(l) |! ─84.86kJ A. |! +137.2 |! kJ B. |! ─137.2 |! kJ C. |! +32.6 |! kJ ─32.6 |! kJ |! - |! Correct |! answer |! ✔B Given |! that: |! 2 |! SO3(g) |! 2 |! SO2(g) |! + |! O2(g); |! ΔHorxn |! = |! +197.8 |! kJ/mol
S(s) |! + |! (3/2) |! O2(g) |! SO3(g); |! ΔHorxn |! = |! ─395.7 |! kJ/mol Determine |! the |! heat |! of |! formation |! for |! SO2. |! A. |! + |! 98.9 |! kJ/mol B. |! + |! 197.8 |! kJ/mol C. |! +691.8 |! kJ/mol ─296.8 |! kJ/mol |! - |! Correct |! answer |! ✔D How |! much |! heat |! is |! absorbed |! in |! the |! complete |! reaction |! of |! 3.00 |! grams |! of |! SiO2 |! with |! excess |! carbon |! in |! the |! reaction |! below? |! ΔH° |! for |! the |! reaction |! as |! written |! is |! +624.7 |! kJ. |! SiO2(g) |! + |! 3C(s) |! SiC(s) |! + |! 2 |! CO(g) |! A. |! 31.2 |! kJ B. |! 1.13 |! 105 |! kJ C. |! 5.06 |! kJ D. |! 1.33 |! 104 |! kJ E. |! 366 |! kJ |! - |! Correct |! answer |! ✔A From |! the |! following |! data |! at |! 25°C: H2(g) |! + |! Cl2 |! 2 |! HCl(g); |! ΔH° |! = |! ─185 |! kJ 2 |! H2(g) |! + |! O2(g) |! 2 |! H2O(g); |! ΔH° |! = |! ─483.7 |! kJ Calculate |! ΔH° |! at |! 25° |! for |! the |! reaction |! below: |!
