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- A 90.0 g piece of metal, initially at 98.6°C, is placed into 120.0 g of water initially at 24.3°C. If the final temperature of the water is 34.0°C, what is the specific heat of the metal? (The specific heat of water is 4.18 J/g. °C).Using the equations 2 C6H6 (1) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g)AH° = -6271 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.6 kJ/mol C (s) + O2 (g) → CO2 (g) AH° = -393.5 kJ/mol Determine the enthalpy for the reaction kJ/mol 6 C (s) + 3 H2 (g) → C6H6 (1). 1 2 3 4 5 6. C 7 8. 9. +/- х 100 LOGiven the information below: 2C(s) + 2H20(g) CH4(g) + CO2(g) AH° = 35.3 kJ 2C(s) + 2H20(g) 2C0(g) + 2H2(g) AH° = 462.6 kJ -> CH4(g) + H20(g)→ CO(g) + 3H2(g) AH° = -61.2 kJ %3D Calculate the enthalpy of reaction for the reaction below (in kJ) Co(g) + H20(g) → CO2(g) + H2(g) -366,1 kJ -488.5kJ -436.7 kJ +488.5 kJ +436,7 kJ +366.1kJ O0 0 O OO
- Given the following information: 2C(s) + 2H20(g)→ CHĄ(9) + CO2(g) AH° = 35.3 kJ C(s) + H20(g) → CO(g) + H2(g) AH° = 231.3 kJ Co(g) + H20(g)→ CO2(g) + H2(g) AH° = -61.2 kJ Find the enthalpy change for the reaction below in kJ CH4(g) + H20(g) CO(g) + 3H2(g) IMPORTANT: Enter both the sign and the value (no units) using 1 decimal placeUsing the equations 2 C6H6 (1) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g)AH° = -6271 kJ/mol C (s) + O2 (g) → CO2 (g) AH° = -393.5 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (g) AH° = -483.6 kJ/mol Determine the enthalpy for the reaction 6 C (s) + 3 H2 (g) → C6H6 (1). kJ/mol 1 3 4 6. C 7 8. 9. + +/- х 100 2.2 NOCI(g) → 2 NO(g) +Cl2(g) AH° =+75.56 kJ 2 NO(g) + 02(g) → 2 NO2(g) AH° =-113.05 kJ 2 NO2(g) → N2O4(g)AH° =-58.03 kJ Compute AH° of N2O4(g) +Cl2(g) → 2 NOCI(g) + O2(g) in kJ. +246.65 -95.52 -246.65 +95.52 +47.76
- Using the equations SrO (s) + CO2 (g) → SrCO3 (s) AH° = -234 kJ/mol 2 Sr(s) + O2 (g) → 2 SrO (s) AH° = -1184 kJ/mol CO2 (g) → C(s) + O2 (g) AH° = 394 kJ/mol Determine the enthalpy (in kJ/mol) for the reaction 2 SrCO: (s) → 2 Sr (s) + 2 C(s) + 3 O2 (g).Using the equations 2 CsHs (l) + 15 Oz (g) → 12 COz (g) + 6 H₂O (g)AH° = -6271 kJ/mol 2 H₂(g) + O₂(g) → 2 H₂O (g) AH° = -483.6 kJ/mol C (s) + O₂(g) → CO₂ (g) AH° = -393.5 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction. 6 C (s) + 3 H₂(g) → C6H6 (1).Calculate AH for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g), from the following data: N2 (g) + O2 (g) → 2 NO (g) AH = -180.5 kJ N2 (g) + 3 H2 (g) → 2 NH3 (g) AH = -91.80 kJ 2 H2 (g) + O2 (g) → 2 H2O (g) AH = -483.6 kJ Select one: O - 1628 kJ O -1995 kJ O 1268 kJ O 755.9 kJ
- From the enthalpies of the reaction H2(g)+F2(g)→2HF(g)AH=-537kJ C(s)+2F2(g) →CF4(g)AH=-680kJ 2C(s)+2H2(g) →C2H4(g)AH=+52.3kJ calculate AH for the reaction of ethylene with F2: C2H4(g)+6F2(g)→2CF4(g)+4HF(g)Given the following data: 2 H2(g) + O2(g) → 2 H20(1) N,O5(g) + H,O(I) → 2 HNO3(1) N2(g) + 3 O2(g) + H2(g) → 2 HNO3(1) AH° = -571.6 kJ AH° = -76.6 k) AH° = -348.2 kJ Calculate the AH° for the reaction: 2 N2(g) + 5 02(g) → 2 N2O5(g)For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. C8H18 (g) + -25 0₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) AH; = ΔΗ What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? 18 -208.5 Incorrect ▲Hixn = -5108.7 kJ/mol kJ/mol