Calculate enthalpy changes for the following: a. 0.069 g of sulfur (rhombic) burns, forming SO₂(g) (AƒH° for SO₂ (g) : Enthalpy change = kJ b. 0.18 mol of HgO(s) decomposes to Hg(l) and O₂(g) (AƒH° for HgO = -90.83 kJ/mol) Enthalpy change c. 2.30 g of NH3(g) is formed from N₂(g) and excess H₂(g) (AƒH° for NH3 = -45.90 kJ/mol) Enthalpy change = KJ d. 1.46 x 10-2 mol of carbon is oxidized to CO₂(g) (AfH for CO₂ = -393.509 kJ/mol) Enthalpy change = = KJ 296.84 kJ/mol) kJ

Calculate enthalpy changes for the following: a. 0.080 g of sulfur (rhombic) burns, forming SO₂(g) (AƒH° for SO₂ (g) Enthalpy change kJ b. 0.33 mol of HgO(s) decomposes to Hg(l) and O₂(g) (AƒH° for HgO = -90.83 kJ/mol) Enthalpy change c. 2.80 g of NH3(g) is formed from N₂ (g) and excess H₂(g) (Aƒ H° for NH3 = -45.90 kJ/mol) Enthalpy change d. 1.36 × 10-2 = Enthalpy change = = mol of carbon is oxidized to CO₂(g) (AƒH° for CO₂ = -393.509 kJ/mol) = == kJ 296.84 kJ/mol)

The value of AH° for the reaction below is 128.1 kJ CH,OH -Co, + 2H (1) 2(g) 2(g) How may kJ of heat are consumed when 10.1 g of H2(g) is formed as shown in the equation? Given that the atomic mass of C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol Show your answers in TWO (2) decimal places. Do not include the units in your final answers.

Calculate the total enthalpy change (kJ) for the following reaction:   H2O (s, 90 g, –10. oC)     -->     H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 kJ/mol.)