Predict the compound in the following pair with the higher decomposition temperature. LiCO3 and NaCO3 Answer: Determine which of the statements below gives reason for your prediction: a. For the decomposition of group 1 carbonates, ArH (M₂O) becomes more endothermic down the group . Group 1 carbonates are relatively stable to heating. LiCO3 is an exception. Lit is a small positive cation with high charge density +

The enthalpy for the formation of 1 mole of NH3(aq)NH3(aq) is -80.29 kJ/molkJ/mol. What is the enthapy for the formation of 3 moles of NH3(aq)NH3(aq)?

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What is the The enthalpy change for the reaction: calcite › aragonite

1. How many kJ of energy are released by 34.65 g of boron? Ti + 2 B -> TiB2  △ H  = 316 kJ/mol   2. How much energy in kJ is released when 14.17 g of aluminum react with an excess of copper oxide? 3 CuO + 2 Al -> 3 Cu + Al2O3  △ H  = 1190 kJ/mol   3. If 36.26 grams of aluminum is heated from 18 oC to 26 oC how much energy was required? sAl = 0.897 J/(gK)

Part A Calculate the enthalpy of the reaction 2NO(g) + O2(9)–→2NO2(9) given the following reactions and enthalpies of formation: A N2(9) + O2(g)→NO2(9), AfH = 33.2 kJ mol 1 B. N2 (9) + ¿O2(9)→NO(g), AfHß = 90.2 kJ mol 1 Express your answer with the appropriate units. • View Available Hint(s) ? A¢H° = Value Units Submit

Calculate the heat of reaction per mole of water if addition of 25.0 mL of 0.101 M A H2SO4 to 50.0 mL of 0.103 M NaOH causes the temperature to rise by 0.99°C. Assume that for both solutions the density is 1.00 g/mol and the specific heat (s) = 4.184 J/g°C. %3D

Using the thermodynamic tables find the enthalpy of formation for BaCO3 (s) a. none of these b. – 1.29 x 103 kJ c. + 314.4 kJ d. – 1219 kJ e. – 628.8 kJ f. – 5.16 x 103 kJ g. – 314.4 kJ

The reaction of CH3OH(g) with N2(g) to give HCN(g), NH3(g), and O2(g) requires 164 kJ/mol of CH3OH(g). Write a balanced chemical equation for this reaction. Include the phases of all species in the reaction.  How much heat is involved in the reaction of 65.0 g of CH3OH(g) with excess N2(g) to give HCN(g) and NH3(g) in this reaction?

2. Please calculate the standard enthalpy of reaction (AHrxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na2O(s) → 2NaNO2 (s) NO(g) + NO₂(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O2(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ = 507.31 kJ/mol AH = -427.14 kJ/mol AH = - 42.68 kJ/mol 34.35 kJ/mol ΔΗ ΔΗ = 44.012 kJ/mol =