Calculate the molar enthalpy with respect to Ti2O3. Balance the equation so Ti2 03 has a "1" and include the molar enthalpy within this new version of the reaction. 2T1203 -> 4Ti + 302 AH = +1200. kJ Is the full equation to use

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)?

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

Using the provided enthalpy of formation, determine the enthalpy for the reaction: 3A (s)+ 2B (I) ->C (I) + 4D(s) substance AH;° (KJ/mol) A (s) -286

From the change in internal energy, AE, given for 40 °C, calculate the change in enthalpy, AH, at the same temperature for the reaction: N202 (g) → N2 (g) + O2 (g) AE = -151.3 kJ O -153.2 kJ -153.8 kJ O -155.2 kJ O -148.7 kJ O -151.3 kJ A Moving to another question will save this response. MacBook Air 吕口 F3 F4 F5 F6 # $4 3. 4 6.

Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction: 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s) This reaction occurs when a mixture of powdered aluminum and iron(III) oxide is ignited with a magnesium fuse. The following enthalpies of formation are known: AH°; for Fe203(s) = -826 kJ AH°; for Al203(s) = -1676 kJ O 1251 kJ O 2502 kJ O-1251 kJ O 425 kJ 850 kJ O- 2502 kJ -850 kJ -425 kJ

16. Use enthalpies of formation given to determine the standard enthalpy of reaction for the following: ed oioege Al2O3 (s) +2 Fe 2 Al (s) + Fe2O3 (s) AH° =??? > AH°r(kJ/mol) -825.5 -1676 17. Use the enthalpies of formation and the enthalpy of reaction given below to determine the enthalpy of formation for solid CaC2. CaC2 (s) + 2 H2O (1) → Ca(OH)2 (s) + C2H2 (g) AH° =-127 kJ AH° (kJ/mol) ??? -286 -986 +227

Write a balanced equation for the reaction between gaseous methane (CH4)(CH4) and fluorine gas to produce gaseous carbon tetrafluoride and gaseous hydrogen fluoride. Include phases. balanced equation:   Calculate the standard enthalpy of reaction (Δ?∘rxn).(Δ⁢Hrxn∘). Use the standard enthalpy of formation values in this table of thermodynamic properties. For carbon tetrafluoride, use Δ?∘f=−933.2 kJ/mol.Δ⁢Hf∘=−933.2 kJ/mol. Δ?∘rxn=Δ⁢Hrxn∘=   Suppose that 0.433 mol0.433 mol of methane gas is reacted with 0.904 mol0.904 mol of fluorine gas. Assuming the reaction occurs at constant pressure, how much heat is released? amount of heat released:

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 =

Calculate the change in enthalpy of the following reaction. ΔH (Fe3O4) = -1120.9 kJ ΔH (Al2O3) = -1669.8 kJ  8Al(s) + 3Fe3O4(s) -> 4Al2O3(s) + 9 Fe(s