(Please explain) Hess Law delta H
Manipulate the data provided to find the ΔHrxnfor the reaction: CH4(s) + 2 O2(g) →CO2(g)+ 2 H2O(l)
(1) 2 CH4(g)+ 3 O2(g) →2 CO(g) + 4 H2O (l) ΔH= −1215 kJ
(2) 2C + O2(g) →2 CO(g) ΔH= −221 kJ
(3) C (s) + O2(g) → CO2(g) ΔH= −394 kJ
I have solved it myself but I am not sure of the answer I have gotten. my answer was about -228.5kj
(Please explain) Hess Law delta H Manipulate the data provided to find the ΔHrxnfor the reaction:...
Use Hess' Law to calculate the ΔH for the following reaction from the data given below. Na2CO3(s) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l) ΔH = _________ Na2CO3(s) → CO2(g) + Na2O(s) ΔH = 319.8 kJ 2NaCl(aq) + H2O(l) → 2HCl(aq) + Na2O(s) ΔH = +348.0 kJ
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l). Use the series of reaction that follows: 1. C(s)+2H2(g)-> CH4(g), delta H= -74.8 kJ 2. C(s)+O2(g)->CO2(g), delta H= -393.5 kJ 3. 2H2(g)+O2(g)-> 2H2O(g), delta H= -484.0 kJ 4. H2O(l)->H2O(g), delta H= 44.0 kJ
Calculate the change in enthalpy (ΔH) for the heat of formation of ethane, C2H6, using Hess' Law and the following reactions:a) 2C(S) + 2O2(g) → 2CO2(g), ΔH = -188 kcalb) C2H6(g) + (7/2)O2(g) → 2CO2(g) + 3H2O(l), ΔH = -373 kcalc) H2(g) + (1/2)O2(g) → H2O(l), ΔH = -68.3 kcal
3. Calculate AG ° of the following reaction: 2C(s) + H 2 (g) → C2H 2 (g) Use Hess' Law, AG ° = AG°ı + AG°2 + AG°3 after manipulating the minor reactions. C2H2 (g) + 5/2 O2 (g) 5/2 O2 (g) → 2 CO2 (g) → 2 CO2 (g) + H20 (1) C(s) + O2 (g) → CO2 (g) H2 (g) + 12 O2 (g) → H20 (1) AG° = -1234 kJ AG° = -394 kJ AG = -237...
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
The next three questions will take you through the calculation of Delta H for the following reaction using Hess's Law. Follow the steps and answer each question in turn. 2BaCO3 (s) -----> 2Ba (s) + O2(g) + 2CO2 (g) AH = ? Given the following reactions and thermochemical data: 1. Bao (s) + CO2 (g) -------> BaCO3(s) AH = - 277.4 kJ 2. 2 Bao (s) -------> 2 Ba (s) + O2(g) AH = + 1096.2 kJ After rearranging as/if...
5. Use the following data to determine the delta H for the conversion of diamond into graphite: C(diamind) (s) + O2(g) = CO2(g) delta H degrees = -395.4 kJ 2CO2(g) = 2 CO(g) + O2(g) delta H degrees = 566.0 kJ 2CO(g) = C(graphite) (s) + CO2 (g) delta H degrees = -172.5 kJ C(diamond) (s) = C(graphite) delta H degrees = ?
4CO(g) + 8H2(g) -----> 3CH4(g) + CO2(g) + 2H2O(l) Use the following data as needed to determine ΔH for this reaction. 1.) C(s) + 1/2O2(g) -----> CO(g) ΔH = -110.54 kJ 2.) CO(g) + 1/2O2(g) -----> CO2(g) ΔH = -282.97 kJ 3.) H2(g) + 1/2O2(g) -----> H2O(l) ΔH = -285.85 kJ 4.) C(s) + 2H2(g) -----> CH4(g) ΔH = -74.85 kJ
The next three questions will take you through the calculation of Delta H for the following reaction using Hess's Law. Follow the steps and answer each question in turn 2Baco, (s) -----> 2Ba (s) + O2(g) + 2CO2 (g) AH = ? Given the following reactions and thermochemical data: 1. BaO (8) + CO2 (g) ----ảy> BaCO3 (5) AH = 274 VI 2. 2 Bao (s) -------> 2 Ba (s) + O2(g) AH + 1096.2 kJ After rearranging as if...
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol, calculate the percent error