Calculate [delta H0 f] in kJ for the equation below using the standard enthalpies of formation...
answer should be in sig figs. LReterences] TUTOR Calculating Enthalpy Change Using the standard formation enthalpies that follow, calculate the standard enthalpy change for this reaction. 2CO(g)+2NO(g)2CO2(g)+ N2(g) AH kJ Species AHo (kJ/mol) -110.5 CO(g) NO(g) CO2(g) 90.3 -393.5
Using the table of standard entropies and enthalpies of formation, calculate AH°, ASº, and AG° for the following reactions at 298.15 K. (Use only the table of standard entropies and standard enthalpies of formation, not the table of standard Gibbs free energies.) kJ AH; () AS; mol-K mol Compound C(s) 5.7 CO(g) -110.5 197.7 The equation SiO2(s) + 2 Mg(s) Si(s) + 2 CO2(g) -393.5 213.8 MgO(s) C2(g) 223.1 H2(g) 130.7 • AH° kJ HCl(g) 186.9 -92.3 • AS° MK...
which of the following statements is/are true concerning a state function Using the standard enthalpies of formation listed below, determine the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) ---> 2Fe(s) + 3C02() AH°-m AH" for Fe2O3(s) --824.2 kJ/mol AH® for CO(g) = -110.5 kJ/mol AH", for CO2(g) - -393.5 kJ/mol
help asap 3. Calculate the standard enthalpy change, Hº, for the following reaction using standard enthalpies of formation. (1 point) 2C2H2(g) + 502(g) → 4CO2(g) + 2H20(1) Standard Enthalpies of Formation AH for C2H2(g) = +226.7 kJ/mol AHfor CO2(g) = -393.5 kJ/mol AH for H2O(l) = -285.8 kJ/mol
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the change in enthalpy for each of these reactions Hrxn [n. Ho(products) - n. Ho(products)] CO (g): -110.5 kJ/mol; CO2 (g): -393.5 kJ/mol CH4 (g): -890.4 kJ/mol H2O (l): -285.8 kJ/mol; H2O (g): -241.8 kJ/mol H2S (g): -20.6 kJ/mol; NO: -90.2 kJ/mol NO2: +33.9 kJ/mol; HCl (g): -92.3 kJ/mol NaOH (s): -426.7 kJ/mol; SO2 (g): -296.8 kJ/mol a) CH4(g) + 2 O2(g) ---> CO2(g) +...
Calculate enthalpy change using standard heats of formation. Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. S(s.rhombic) + 2CO(g) +SO2(g) + 2C(s.graphite) Hºrn Species AH% (kJ/mol) CO(g) -110.5 SO2(g) 296.8
Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. S(s,rhombic) + 2CO(g)— SO2(g) + 2C(s,graphite) AH°rxn- KJ Species AH®(kJ/mol CO(g) -110.5 SO2(g) -296.8 Check & Submit Answer Show Approach
7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s) + O2(g) + CO2(g) b. S(s) + O2(g) → SO2(e) C. CS2() + 302(g) → CO2(g) + ' 250 (6) AH° = -393.5 kJ/mol AH° = -296.4 kJ/mol AH° = -1073.6 kj/mol (the standard state of the element Sulfur is S(s))
Calculate the AH formation of octane, CBH1B (), given that the enthalpy of combustion of octane is -5471 kl/mol and the standard enthalpies of formation of H20 () and CO2 (g) are -393.5 kJ/mol and -285.8 kJ/mol respectively.
need help with 2. Use the following enthalpies of formation to calculate an approximate enthalpy of reaction, AHrxn for: (5 pts) C3H8 (g) + 502 (g) → 3CO2 (g) + 4 H20 (1) C(s) + O2 (g) - CO2 (g); AH = - 393.5 kJ/mol H2(g) + 42 02 (g) - H20 (1); AH = - 285.5 kJ/mol 3 C(s) + 4 H2(g) → C3H8 (g); AH r = - 103.8 kJ/mol