Useful info 1 bar = 10° Pa 1 atm = 1.013bar R = 8.314 J/K-mol NA = 6.022x1023 mol = 8.206x10 L-atm/K-mol 3 = 8.206x10° m²-atm/K-mol 8 = 9.807 m/s? Pm[H2O] = 1.00 g/mL = 760 Torr = 62.36 L-Torr/K-mol 1 mbar = 10 bar 1J = 10² L-bar = 9.870×10³ L-atm= 0.2390 cal = 10² cm= 10° mm= 10° µm = 10° nm=101º A 1J = 1 Pa-m³ 1 L-atm = 101.3 J 1 m³ = 10³ L = 106 cm³ At 298 K (only): %3D RT = 2.478 kJ/mol (= 24.46 L-atm/mol) Physical Properties of Selected Substances mol. wt. ΔΗ Sm J/(mol·K) J/(mol·K) Cp,m AHus melting temp AHap boiling temp kJ/mol g/mol 39.9 kJ/mol K kJ/mol K 154.84 Ar(g) C(s,grpht.) CH;OH(1) CH;OH(g) CH4(g) CO(g) CO,(g) H,(g) H,O(1) H,O(g) NH;(g) O2(g) Properties of pure phases are for standard conditions of 298 K and 1 atm. Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm. 20.786 12.01 8.53 32.04 -238.66 81.6 3.16 175.2 35.29 337.2 32.04 -200.66 43.9 16.04 -74.8 35.3 0.94 91 8.2 112 28.0 -110.53 29.14 44.0 -393.5 213.74 37.11 2.0 116.1 28.8 18.0 -285.8 69.9 75.3 6.0 273 40.6 373 18.0 -241.8 188.8 33.6 18.0 -46.1 192.4 35.1 5.7 195 23.3 240 32.0 205.1 29.4 Integrals Equations of state xn+1 x" dx ;n + -1 RT a ; van der Waals V2 n + 1 Vm In x В RT 1 + Vm + ... ; virial Vm 1 dx 1 - In (аx — b) ax a Nomenclature – but, when in doubt, write it out! AH Change in enthalpy for an arbitrary process (units of energy) AHm Change in enthalpy for an arbitrary process, per mole (energy/mole) AH, or AHn Standard molar enthalpy of reaction, per mole, between separated products and reactants, each in the standard states for the phases specified and at the specified temperature. (energy/mole) rxn 10

Determine the enthalpy change, AH, in kJ, for the following reaction: CS2 (1) + 302 (g) --> CO₂ (g) + 2SO2 (g) given the following thermochemical equations: C(s) + O₂ (g) --> CO₂ (g) ΔΗ = 91.2 kJ S (s) + O₂ (g) --> SO₂ (g) ΔΗ = -382 kJ C(s) + 2S (g) --> CS₂ (1) Do not report units in your answer. Report your answer to one decimal place and include the correct sign in your answer. AH = 82.6 kJ

Use the thermochemical equations shown below to determine the enthalpy for this reaction: 2 H2O(g) + 2 Cl2(g) →4 HCl (9) + O2(g) ΔΗ xn Information: COCI 2(g) + H2O(l) → CH2Cl2(1) + O2(g) AH = 19 kJ H2O(g) →H2O(l) AH = -44 kJ HCI (g) 1/2 H2(g) +1/2 Cl2(g) AH = 92 kJ CH2Cl2(1) + H2(g) + 3/2 O2(g) → COCI 2(g) + 2 H2O (1) AH=-161k]

1. The enthalpy changes of the following reactions Can be measured: Co H. (g) + 7/2 Q₂ (g) → 2 CO₂ (g) + 3 H ₂ O ( ) соно A₁ H° = - 1428.7 KJ/mol-rxn f C₂ H ₂ OH (g) + 3 Q₂ (g) →) 2 CO₂ (g) + 3 H ₂ O (g) Arto= ° = -1277 kJ/mol-rxn a Use these values and Hess's law to determine the for the reaction. ½/2 C ₂ H 6 (g) + ½z O₂ (g) → C₂ H₂ OH (g) en On thalpy chang ks/mol-cox Enthalpy Change = 000 20 * LANCEEL

Write a balanced equation for the reaction between gaseous methane (CH4)(CH4) and fluorine gas to produce gaseous carbon tetrafluoride and gaseous hydrogen fluoride. Include phases. balanced equation:   Calculate the standard enthalpy of reaction (Δ?∘rxn).(Δ⁢Hrxn∘). Use the standard enthalpy of formation values in this table of thermodynamic properties. For carbon tetrafluoride, use Δ?∘f=−933.2 kJ/mol.Δ⁢Hf∘=−933.2 kJ/mol. Δ?∘rxn=Δ⁢Hrxn∘=   Suppose that 0.433 mol0.433 mol of methane gas is reacted with 0.904 mol0.904 mol of fluorine gas. Assuming the reaction occurs at constant pressure, how much heat is released? amount of heat released:

The standard enthalpy change for the following reaction is -135 kJ at 298 K. 1/2 N2(g) + 1/2 H2(g) + 3/2 O2(g) HNO3(g)       ΔH° = -135 kJ What is the standard enthalpy change for the reaction at 298 K? N2(g) + H2(g) + 3 O2(g)2 HNO3(g) kJ

Calculate ΔHo for the process ½ N2(g) + ½ O2(g) → NO(g) from the following information N2(g) + 2 O2(g) → 2 NO2(g)  ΔHo = -105.8 kJ/mol 2 NO(g) + O2 → 2 NO2(g)  ΔHo = -216.7 kJ/mol

A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH),(s)-Al,0,(s) + 3H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 3AI,0,(s) + 9H,0() 6Al(OH),(s) Al,0,(s) + 3H,0() 2Al (OH), (s) Al(OH),(6) - Al,0,(0) + ,00 1 Al,0,(5) + H,0() O kJ Explanation Check 2021 McGra M B

Which of the reactions are exothermic?

Among the equations below, indicate all those that are exothermic: i. HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l)                    ∆H = -53 kJ ii. Fe3O4(s) + CO(g) + 38 kJ → 3FeO(s) + CO2(g) iii. CaO(s) + H2O(l) → Ca(OH)2(aq) + 65,2 kJ iv. H2O2(l) → H2(g) + O2(g)                                                 ∆H = 188 kJ v. NaOH(s) + HCl(l) → NaCl(s) + H2O(l)                              ∆H = -178 kJ