Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction is 5.42  × 10–4, and ΔH∘∘ for the reaction is 180.6 kJ. $$N2​(g)+O2​(g)2NO(g)     1st attempt   See Periodic Table What is the value of Kc at 1000.0°C?

Calorimetry: Question #3 Octane, C3H18 , is a constituent of gasoline, and burns in the presence of oxygen to produce water and carbon dioxide: 2 C3H18 (1) + 25 O2(g) → 16 CO2(9) + 18 H2O1) ΔΗ kJ/2mol %3D rxn C3H18 (1) When a 1.00-gram sample of octane is burned in a bomb calorimeter the temperature of the water and the calorimeter rises from 25.00°C to 33.20°C. If the heat capacity, Cbomb cal, of the empty bomb calorimeter is 837 J/°C, and the mass of the water is 1.200 kg: a) Calculate the heat, q, transferred, during the combustion, to the calorimeter: 6.86 kJ (calorimter) + qbomb cal = Cbomb cal • AT b) Calculate the heat, q, transferred, during the combustion, to the water: 41.2 kJ (1.200 kg H20) + 9H20 = + mH20 • AT • SH2O c) Calculate the enthalpy change (AHº rxn = kJ/2mol) for this reaction (2 mol of C3H18 (1): [ Select ] kJ/2 mol C3H18 (1)

The standard enthalpy change for the following reaction is 851 kJ at 298 K. 2 NaOH(s) 2 Na(s) + O2(g) + H2(g) AH° = 851 kJ What is the standard enthalpy change for this reaction at 298 K? Na(s) + 1/2 O2(g) + 1/2 H2(g) NaOH(s) kJ Submit Answer Retry Entire Group 9 more group attempts remaining

Using Hess's law, what is AHf rxn for the following reaction? NO(G) + O(g) – NO2(9) NO(g) + O3(9) – NO2(9) +O2(9) AH xn = -198.8 kJ/mol Og(9) – 3/2 02(9) AHrxn = -142.2 kJ/mol 02(9) → 20(9) AH Prxn = +498.8 kJ/mol -839.8 kJ/mol -306.0 kJ/mol 394.9 kJ/mol 157.9 kJ/mol O 442.3 kJ/mol QUESTION 8 Octane (C3H18) undergoes combustion according to the following thermochemical equation. 2C8H18() + 2502(g) – 16CO2(g) + 18H20() AH°rxn = -1.0940 x 104KJ/mol What is the standard enthalpy of formation of liquid octane? AH°{(CO2(g)) = -393.5 kJ/mol and AH°F{H2O(1)) = -285.8 kJ/mol 495 kl/mol O -250 kJ/mol -495 kJ/mol -10,940. kJ/mol -2188 kJ/mol

When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat (in kJ) is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg?   ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05

Using the equation labels in the laboratory procedure, which of the following illustrates the correct calculation for ΔH4? (1) C(s) + 1/2O2(g) → CO(g) ∆H1 = ? (2) C(s) + O2(g) → CO2(g) ∆H2 = -395.7 kJ/mol   (3) CO(g) + 1/2O2(g) → CO2(g) ∆H3 = -283.2 kJ/mol   Summing reactions appropriately to determine ∆H1:   C(s) + O2(g) → CO2(g) ∆H2 = -395.7 kJ/mol (Reaction 2)   CO2(g) → CO(g) + 1/2O2(g) (-∆H3) = 283.2 kJ/mol (reverse of 3) Sum: C(s) + 1/2O2 → CO(g) -395.7 + 283.2 = -112.5 kJ/mol   Determination of the Enthalpy of Sublimation and Decomposition of NH4Cl In the laboratory experiment today, the heat of sublimation and decomposition of NH4Cl(s) will be determined. The process is represented by Equation 4.   (4) NH4Cl(s) → NH3(g) + HCl(g) ∆H4 = ?   Solid ammonium chloride sublimes (i.e., changes from a solid to a gas) at 340oC and decomposes to gaseous ammonia and hydrogen chloride. ∆H4 is obtained via mathematical manipulation of four equations and the enthalpy changes corresponding to…

9:47 Unanswered • 1 attempt left • Due on Oct 20, 7:00 PM A nickel at 30 °C is dropped into a glass of 15.0 g soda at 3.0 °C, if the heat capacity of the nickel is 4.40 J/°C, the heat capacity for the glass is 11.1 J/°C, and the soda has the same specific heat capacity as water (4.184 J/g°C), what is the final temperature of the mixture? A 8.3 °C В 5.6 °C C 4.5 °C 3.4 °C E e. 1.7 °C A Submit

Use the following information to answer the question:   What is the ΔH (in kJ/mol) for the following reaction? (Show work) CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g) Given: C(s) + O2(g) → CO2(g); ΔHf = -393.5 kJ/mol S(s) + O2(g) → SO2(g); ΔHf = -296.8 kJ/mol C(s) + 2 S(s) → CS2(l); ΔHf = 87.9 kJ/mol

The standard enthalpy change for the following reaction is 1.11×103 kJ at 298 K. 2 BaO(s)2 Ba(s) + O2(g)       ΔH° = 1.11×103 kJ What is the standard enthalpy change for this reaction at 298 K? Ba(s) + 1/2 O2(g) BaO(s) _____kJ