When 12.0 g (0.100 mol) of MgSO,(s) is dissolved in water in a constant pressure calorimeter, the temperature increases from 20.0 to 38.2°C. The heat capacity of the calorimeter and all its contents is 500. JK-1. What is the enthalpy of dissolution of magnesium sulfate (in kJ mol-1)? А 107 B 91.0 -91.0 D -107

For the reaction below, ΔrH° = −3307.9 kJ mol−1. What is the standard enthalpy of formation of FeS2(s)? 4 FeS2(s) + 11 O2(g)  ⟶ 2 Fe2O3(s) + 8 SO2(g) Give your answer in kilojoules per mole (kJ mol−1). Data: Substance Standard enthalpyof formation (in kJ mol−1) Fe2O3(s) −833.1 SO2(g) −297.0 Please double check your answer.

For each reaction equation, calculate the internal energy change, ΔE, of the reaction at 25 ∘C   2H2(g)+O2(g)⟶2H2O(l)Δ?=−571.6 kJ   Δ?=   kJ   H2(g)+Cl2(g)⟶2HCl(g)Δ?=−184.6 kJ/mol   Δ?=   kJ

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. Mg(OH), (s) + 2 HCI(g) → MgCl, (s) + 2 H,O(g) AHixn kJ

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. C₂H₂ (g) + 50₂ (g) - AHixn = 3 CO₂(g) + 4 H₂O(g) kJ

In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq)     ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.

What is ΔHrxn if mixing 50.0 mL of 0.500 M HCl (aq) with 50.0 mL of 0.500 M NaOH (aq), both initially at 24.0 °C results in a Tmix of 27.3 °C?  Assume that the reaction goes 100%  HCl (aq) + NaOH (aq) → H2O (l) + NaCl(aq) **answer in kJ/mol of H2O produced

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ

Calcium ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) Ca (s) 0 0 41.4 Ca (g) 178.2 144.3 158.9 Ca2+ (g) 1925.9     CaC2 (s) -59.8 -64.9 70.0 CaCO3 (s, calcite) -1206.9 -1128.8 92.9 CaCl2 (s) -795.8 -748.1 104.6 CaF2 (s) -1219.6 -1167.3 68.9 CaH2 (s) -186.2 -147.2 42.0 CaO (s) -635.1 -604.0 39.8 CaS (s) -482.4 -477.4 56.5 Ca(OH)2 (s) -986.1 -898.5 83.4 Ca(OH)2 (aq) -1002.8 -868.1 -74.5 Ca3(PO4)2 (s) -4126.0 -3890.0 241.0 CaSO4 (s) -1434.1 -1321.8 106.7 CaSiO3 (s) -1630.0 -1550.0 84.0       Carbon ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) C (s, graphite) 0 0 5.7 C (s, diamond) 1.9 2.9 2.4 C (g) 716.7 671.3 158.1 CCl4 (l) -135.4 -65.2 216.4 CCl4 (g) -102.9 -60.6 309.9 CHCl3 (l) -134.5 -73.7 201.7 CHCl3 (g) -103.1 -70.3 295.7 CH4 (g) -74.8 -50.7 186.3 CH3OH (g)…

11. What is the ΔHº-value for the dissolution of NaOH (s) to yield 1.00... m NaOH (aq), given:      Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (s)              ΔHfº = -425.9 kJ/mol   Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (aq, 1 m)    ΔHfº = -469.2 kJ/mol     Multiple Choice   -895.1 kJ/mol   -43.3 kJ/mol   +1.102 kJ/mol   +43.3 kJ/mol   +895.1 kJ/mol