7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s)...
Calculate the standard enthalpy of formation of CS2() given that AH=-393.5 kJ/mol AHo = -296.4 kj/mol a. C(s) + O2(g) CO2lg) b. S(s) +O2(g). SO2(g) AH = -1073.6 kj/mol C. CS2(I)+302(g) Co2lg) + 2S02(B)
PLEASEEE HELPP ASAP 7- (15 pts) Calculate the standard enthalpy of formation of CS,() given that AH 393.5 kJ/mol AH- 296.4 kj/mol a. C(s) Oz(g) COlg) b. S(s) O,(g). SOlg) c. CS)()30 (g) CO,(B ) + 2SO;(g) + AH° -1073.6 kj/mol (the standard state of the element Sulfur is S(s)
Using Hess's Law, determine the enthalpy change of the following reaction. CS2(1) + 3 O2(g) --> CO2(g) + 2 SO2(g) C(s) + O2(g) --> CO2(g) AH = -393.5 kJ/mol S(s) + O2(g) --> SO2(g) AH = -296.8 kJ/mol C(s) + 25(s) --> CS2(8) AH = +87.9 kJ/mol -899.2 kJ O-778.2 kJ -602.4 kJ - 1075.0 kJ
Enter your answer in the provided box Use the following data to calculate ΔΗο for CS20: C(graphite)+ O2(8)-Co2() S(rhombic) +02(g) → SO2(g) CS2(0) + 302(8) CO2(8) + 2S02(3) o AH =-393.5 kJ/rnol rxn AH296.4 kJ/mol rxn AHorn =-1073.6 kJ/mol 0
4. Sodium lamps are commonly used to illuminate highways because of their intense yellow- orange emissions at 589 nm a. Calculate the energy, in joules, of one photon of this light. b. Calculate the energy, in kilojoules, of one mole of such photons 5. What is the de Broglie wavelength (in nm) associated with a 2.5 g Ping-Pong ball traveling at 15.6 m/s? 6. What are the possible values of I and what are the possible subshells for an e...
3. (14 pts.) The standard molar enthalpy of formation of Fe,Oxs is AH = -8242 kJ/mol, and the standard molar enthalpy of formation of SO2(g) is AH = -296.8 kJ/mol (both at 298 K). Use this information, along with the standard molar enthalpy change of the following reaction at 298K, 2 FeS21s) + 11/2O2(g) → Fe2O3 + 4 SO2(g) AH = -1655 kJ/mol To determine the standard molar enthalpy change of the reaction shown below are 298 K: Fe(s) +...
Find the enthalpy change for the reaction CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g) when: C(s) + O2(g) → CO2(g) ΔHf = -393.5 kJ/mol S(s) + O2(g) → SO2(g) ΔHf = -296.8 kJ/mol C(s) + 2 S(s) → CS2(l) ΔHf = 87.9 kJ/mol
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = −296.8 kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol A) Calculate the standard enthalpy change for the following reaction CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) ΔH° rxn = -1075 kJ/mol B) Using the equation and standard enthalpy change for the reaction (from part A), calculate the amount of heat produced or consumed when 3.2 mol of CS2 reacts with excess...
Calculate the standard enthalpy of formation of solid calcium carbonate (CaCO3) using the following thermochemical information: Calculate the standard enthalpy of formation of solid calcium carbonate (CaCo3) using the following thermochemical information: 2 Cao(s) 2 Ca(s) O2(g) AH 1270.2 kJ C(s) O2 (g) CO2 (g) AH 393.5 kJ AH 178.3 kJ CaO(s) CO2 (g) CaCO3(s) kJ AH
7. The enthalpy of combustion of C to CO2 is –393.5 kJ/mol C, and the enthalpy of combustion of Co to CO2 is -283.0 kJ/mol CO: C(s) + O2(g) + CO2(g) AH = -393.5 kJ CO(g) + 102(9) CO2(g) AH = -283.0 kJ Using these data, calculate the enthalpy of combustion of C to CO: C(s) + O2(g) → CO(g) AH = ? Answer: -110.5 kJ