ΔHrxno = [ΔHfo (products) - ΔHfo (reactants)]
ΔHrxno = [4 *ΔHfo (Al(s)) + 3 *ΔHfo (O2(g)] – [2 *ΔHfo (Al2O3(s)) ]
3.35 * 10^3 = [4 * 0 + 3 * 0] - [2 * ΔHfo (Al2O3(s))]
or
ΔHfo (Al2O3(s)) = - 1.675 * 10^3 KJ / mole (answer)
References Use the References to access important values if needed for this question. The standard enthalpy...
thank you! Ricrencesi Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -234.6 kJ 2502(g) + O2(g) 2503(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of SO3(e) is kJ/mol Submit Answer Retry Entire Group 2 more group attempts remaining TReview Topics [References Use the References to access important values if needed for...
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References Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)—1C4H10(g) AH° = -125.6 kJ (2) C2H2(g) →2C(s) + 2H2(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C2H4(E) + H2(9) >C_H10(8) AH° = ? Submit Answer