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Must show steps to earn credit. Calculate ΔH° for this process: Sb(s) + 5/2 Cl2(g) ⟶...
Calculate ΔH⁰298 (in kJ) for the process Co3O4(s) → 3 Co(s) + 2 O2(g) from the following information. Co(s) + 1/2 O2(g) → CoO(s) ΔH⁰298 = −237.9 kJ 3 Co(s) + O2(g) → Co3O4(s) ΔH⁰298 = −177.5 kJ Please show detailed work and an explanation.
Calculate ΔH⁰298 (in kJ) for the process Co3O4(s) → 3 Co(s) + 2 O2(g) from the following information. Co(s) + 1/2 O2(g) → CoO(s) ΔH⁰298 = −237.9 kJ 3 CoO(s) + 1/2 O2(g) → Co3O4(s) ΔH⁰298 = −177.3 kJ Please show detailed work and an explanation.
Using Hess's Law, calculate ΔH°R Equation: B2H6 (g) + 6 Cl2 (g) --> 2BCl3 (g) + 6 HCl (g) Given these 3 equations: (please show all work) BCl3 (g) + 3H2O (l) --> H3BO3 (g) + 3HCl (g) (ΔH°R = -112.5 KJ/mol BCl3) B2H6 (g) + 6H2O (l) --> 2H3BO3 (g) + 6H2 (g) (ΔH°R = -493.4 KJ/mol B2H6) H2 (g) + Cl2 (g) --> 2HCl (g) (ΔH°R = -184.6 KJ/mol H2)
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
Calculate the value of ΔH° for the following reaction: P4O10(s) + 6PCl5(g) ---> 10Cl3PO(g) P4(s) + 6Cl2(g) ---> 4PCl3(g) ΔH° = -1225.6 kJ P4(s) + 5O2(g) ---> P4O10(s) ΔH° = -2967.3 kJ PCl3(g) + Cl2(g) ---> PCl5(g) ΔH° = -84.2 kJ PCl3(g) + (1/2)O2(g) ---> Cl3PO(g) ΔH° = -285.7 k please explain well i do not understand these kind of problems
1) CH4(g)+2O2(g)→CO2(g)+2H2O(l)ΔHrxno=−889.1kJmol–1 ΔHfoH2O(l)=–285.8kJmol–1ΔHfoCO2(g)=–393.3kJmol–1 What is the standard heat of formation, ΔHfo, of methane, CH4(g), as calculated from the data above? 2) How much heat, in kilojoules, must be added to a 75.0–g iron block with a specific heat of 0.449 J/g°C to increase its temperature from 25 °C to its melting temperature of 1535 °C? 3) Calculate ΔH298o for the process Sb(s)+52Cl2(g)→SbCl5(g) from the following information: Sb(s)+32Cl2(g)→SbCl3(g)ΔH298o=−314kJ 4) The oxidation of the sugar glucose, C6H12O6, is described by the following...
A chemist measures the enthalpy change ΔH during the following reaction: 2Na (s) + Cl2 (g) → 2NaCl (s) =ΔH−822.kJ Use this information to complete the table below. Round each of your answers to the nearest /kJmol . A chemist measures the enthalpy change AH during the following reaction: 2Na(s) + Cl2(g)→2 NaCl(s) NH=-822. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol reaction △H kJ NaCl(s) → Na(s) + Cl2(g)...
c. Calculate ΔH° for the process Co3O4(s)→3Co(s) + 2O2(g) from the following information: Co(s) + 1/2O2(g)→CoO(s) ΔH° = -237.9kJ 3CoO(s) +1/2O2(g)→Co3O4(s) ΔH° = -177.5k d. Calculate the standard molar enthalpy of formation of NO(g) from the following data: N2(g) + 2O2 →2NO2(g) ΔH° = 66.4 k. 2NO(g) + O2 →2NO2(g) ΔH° = -114.1 kJ
Given the standard enthalpy changes for the following two reactions: (1) Sn(s) + Cl2(g) ------> SnCl2(s) . ΔH° = -325.1 kJ (2) Sn(s) + 2Cl2(g)-----> SnCl4(l) . ΔH° = -511.3 kJ what is the standard enthalpy change for the reaction: (3) SnCl2(s) + Cl2(g) ------> SnCl4(l) . ΔH° = ? _____kJ
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ