Compute AH,1000 of HCI(g) from enthalpies of formation data and these Cpm/[J/(mol K)] expressions, which hold from 298 K to 1500 K. 27.14 + 0.009274 (T/K) – 1.381 (10-5 T2/K²) + 7.645 (10-9 T³/K³) | 26.93 + 0.03384 (T/K) – 3.896 (10-5 T²/K²) + 15.47 (10-9 T³/K³) 30.67 – 0.007201 (T/K) – 1.246 (10-5 T²/K²) – 3.898 (10-9 T³/K³) for H,(g), Cl,(g), and HCI(g), in that order.

Compute AH,1000 of HCI(g) from enthalpies of formation data and these Cpm/[J/(mol K)] expressions, which hold from 298 K to 1500 K. 27.14 + 0.009274 (T/K) – 1.381 (10-5 T2/K²) + 7.645 (10-9 T³/K³) | 26.93 + 0.03384 (T/K) – 3.896 (10-5 T²/K²) + 15.47 (10-9 T³/K³) 30.67 – 0.007201 (T/K) – 1.246 (10-5 T²/K²) – 3.898 (10-9 T³/K³) for H,(g), Cl,(g), and HCI(g), in that order.

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

Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids cation anions Cl- -131.228 I- -51.57 NO3- -108.74 SO4-2 -744.53 Na+ -261.905 -384.138 -286.06 -367.00 -3646.85 W10 ∆G°f of water = -237.129 kJ/mol Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt). Observations (Rxn or No Rxn). S or support and R for Refute Cations Anions Cl- I- NO3- SO4-2 Na+(∆G°rxn) Na+ (∆Grxn) Na+ (ppt or no ppt) Na+ (Rxn or No Rxn) NO RXN NO RXN NO RXN NO RXN Na+ (S or support and R for Refute)
Table 2. Gibbs Free Energies of formation (kJ), ∆G°f, for Ions in 1M Solution and Ionic Solids cation anions Cl- -131.228 I- -51.57 NO3- -108.74 SO4-2 -744.53 Ba+2 -1296.32 W2 -663.9 -796.59 -1362.2 ∆G°f of water = -237.129 kJ/mol Calculated values of ∆G°rxn and the ∆Grxn of each box, Predicted results (ppt or no ppt). Observations (Rxn or No Rxn). S or support and R for Refute Cations Anions Cl- I- NO3- SO4-2 Ba+2(∆G°rxn) Ba+2 (∆Grxn) Ba+2 (ppt or no ppt) Ba+2 (Rxn or No Rxn) NO RXN NO RXN NO RXN RXN Ba+2 (S or support and R for Refute)
Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.
For the dissolution of LiCl in water, ΔHsoln = -37 kJ/mol.Which term would you expect to be the largest negativenumber: ΔHsolvent, ΔHsolute, or ΔHmix?
You have a calorimeter with a heat capacity of 0.426 kJ/ºC. You combine 50.0 mL 1.50 M NaA (A- = conjugate base of weak acid HA) with an equal volume of HCl of higher molarilty. The temperature changes from 18.6 ºC to 21.1 ºC. What is ΔHºdissoc for the dissociation reaction of HA, in kJ?
Determination of enthalpy of neutalisation Ccal=20 J/°C Volume of HCl = 150 ml Initial temperature of HCl = 30 °C Volume of NaOH = 149 ml Initial temperature of NaOH = 30 ° C Final Solution Temperature = 45 °C Moles of H+ = .220 mol Moles of OH- = .221 mol Limitng reagent = OH- Heat transfer of solution = ___________|Kj Enthalpy of neutralisation per mole of limiting reagent = _____________________|kj/ mol
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
Determine the standard enthalpy of formation ∆f Hº (in kJ/mol) for HI (g) given that the enthalpy of thereaction 2 HI (g) ---> H2 (g) + I2 (s), is delta H of the reaction = - 53.0 kJmol-1
just to verify the answer rto 1 is increasing and 2 is increasing>??
What is the heat of precipitation of barium sulphate if volume of both reactants sodium sulphate and barium nitrate was 50 cm3 and concentration was 1.0 moldm-3. Temperature increase were 5oC. c = 4.2J/KgK
50.0 mL of 1.00 M HCl is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriemeter constant (K cal ) of 17.3 J/^ C . A change in temperature was observed from 26.0C to 32.6^ ( C. What is the heat of reaction per mole of KOH? (Assume a solution density of 1.00g / (mL) and specific heat capacity of 4.18 J/g^ C .)
Calculate the standard enthalpy of reaction, Δ?∘rxn,ΔHrxn∘, of each of the given acid–base neutralization reactions involving the strong base KOH.KOH. The standard enthalpy of formation data are provided. Compound or Ion Standard Enthalpy of Formation (kJ/mol) KOH(aq)KOH(aq) −482.4 H2O(l)H2O(l) −285.8 HClO3(aq)HClO3(aq) −98.4 KClO3(aq)KClO3(aq) −349.5 HBr(aq)HBr(aq) −121.0 KBr(aq)KBr(aq) −372.1 NH+4(aq)NH4+(aq) −132.5 NH3(aq)NH3(aq) −80.3 K+(aq)K+(aq) −251.2 1. HClO3(aq)+KOH(aq)⟶KClO3(aq)+H2O(l) Δ?∘rxn=______kJ/mol 2. HBr(aq)+KOH(aq)⟶KBr(aq)+H2O(l) Δ?∘rxn=______kJ/mol 3. NH+4(aq)+KOH(aq)⟶NH3(aq)+K+(aq)+H2O(l) Δ?∘rxn=______kJ/mol Based on the Δ?∘rxnΔHrxn∘ values, what is the most likely conclusion about the strength of the acids? a. HClO3(aq) and HBr(aq) are strong acids, and NH4+(aq) is a weak acid. b. HClO3(aq) and HBr(aq) are weak acids, and NH4+(aq) is a strong acid. c. ,HClO3(aq), HBr(aq), and NH4+(aq) are all strong acids. d. HClO3(aq),…