estimate the enthalpy change for the following reaction: CH3OH(g) + HI(g)CH3I(g) + H2O(g)

Calculate the enthalpy change (in kJ/mol) for the combustion of CS2 (1) using the enthalpy values given in the table. CS₂ (1) + 302 (g) → CO₂ (g) + 2 SO2 (g) AH in kJ/mol Reaction C(s) + O₂ (g) →→→ CO₂ (g) S (s) + O₂ (g) →→→ SO₂ (g) C(s) +2S (s) →→→ CS₂ (1) −393.6 -296.8 +87.9

What is the enthalpy change for the following reaction? SiCl 4 (l)+2H 2 (g) Si(s)+4HCl(g)

Calculate the enthalpy change for the following reaction 2H2S (g) + SO2 (g) → 3S (s) + 2H2O (g) from the following equations:  (1) H2O(g) → H2(g) + 1/2 O2(g) Ho = 241.8 kJ (2) H2S(g) → H2(g) + S(s) Ho = 20.6 kJ ( 3) S(s) + O2(g) → SO2(g) Ho = - 296.8 kJ

Consider the following two reactions and the corresponding enthalpy changes: CH4(g) +2 O2(g)→ CO2(g)+2 H2O(I), ΔΗ 2 CH4(g) + O2(g) 2 CH3OH(I), ΔΗ2 Express the enthalpy change for the third reaction 2CH3OH(I)+3O2(g)-2CO2(g) + 4H2O(g), ΔΗ in terms of ΔΗ1 and ΔΗ2· Ο ΔΗ3=2ΔΗ2 - ΔΗ Ο ΔΗ = ΔΗ + ΔΗ Ο ΔΗ3=ΔΗ - ΔΗ2 Ο ΔΗ3 = 2ΔΗ1 +ΔΗ2 ΔΗ3 = 2ΔΗ - ΔΗ

Hydrazine is an inorganic compound with the chemical formula N2H4. The reaction of hydrazine with chlorine trifluoride has been used in experimental rocket motors in the reaction below: 3N2H4 (1) + 4CIF3 (g) → 3N2 (g) + 12HF (g) + 2C12 (g) Calculate enthalpy change for the reaction given the following: (1) 2CIF3 + 2NH3 → N2 + 6HF + Cl2 (2) N2H4 + O2 → N2 + 2H2O (3) 4NH3 + 302→ 2N2 + 6H20 AH°= -1196 kJ AH°= - 622 kJ AH° = - 1530 kJ

Find the enthalpy change for the reaction below, given the following reactions and their respective ΔHrxn values:                              PCl5(g)  →  PCl3(g)  +  Cl2(g)    ΔH-? P4(s)  +  6Cl2(g)  →  4PCl3(g)            ΔH = -2439 kJP4(s)  +  10Cl 2(g) → 4PCl5(g)           ΔH = -3438 kJ(A)   1490 kJ          (B)   249.8kJ          (C)   372.5             (D)  none of those. If so, what is your answer?

Calculate the enthalpy of the following reaction: HCl + NaOH → NaCl + H2O ΔH HCl= -92.3 kJ/mol NaOH= -426.7 kJ/mol NaCl= -411 kJ/mol H2O= -286 kJ/mol Reaction: ΔH=    kJ/mol

Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is H2 (9) +O2 (9) → H2O2 (1) Calculate the enthalpy change using the following data: 2H2O2 (1) → 2H2O(1) +O2 (g); AH=-196.0 kJ H2 (g) + O2(g)→ H20(1); AH -285.8 kJ AH kJ %3D

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs