Use the following information and hess's law to find
the enthalpy change for the reaction
C(g) + O2(g) => CO2(g)
reaction 1: 2CO(g) + O2(g) => 2CO2(g) ΔH = -566
kj
reaction 2: 2C(g) + O2(g) => 2CO(g) ΔH = -1655 kj
Use the following information and hess's law to find the enthalpy change for the reaction C(g)...
Use Hess’s Law to find the standard enthalpy change for the reaction CO2(g) → C(s) + O2(g) using only the following information. Show all your work, including any equations you use to obtain your answer and showing clearly how you obtained that answer. (3 pts.) H2O(l) → H2(g) + 1/2O2(g) C2H6(g) → 2C(s)+ 3H2(g) 2CO2(g) + 3H2O(l) → C 2H6(g) + 7/2O2(g) ∆Ho (kJ) 643 kJ 190.6kJ 3511.1 kJ
a) Use Hess's law to calculate the enthalpy change for the reaction: 3C(s) + 4H2(g) + ½O2(g) → C3H8O(l) Given the following thermochemical equations: 2C3H8O(l) + 9O2(g) → 6CO2(g) + 8H2O(l) ΔH = -4042.6 kJ/mol C(s) + O2(g) → CO2(g) ΔH = -393.51 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH = -285.83 kJ/mol (in kJ/mol) A: -267.7 B: -302.6 C: -341.9 D: -386.3 E: -436.5 F: -493.3 G: -557.4 H: -629.9 b) Define if the following statement is an endothermic process or exothermic...
Learning Goal: To understand how to use Hess's law to find the enthalpy of an overall reaction. The change in enthalpy, ΔH, is the heat absorbed or produced during any reaction at constant pressure. Hess's law states that ΔH for an overall reaction is the sum of the ΔH values for the individual reactions. For example, if we wanted to know the enthalpy change for the reaction 3Mn+3O2→3MnO2 we could calculate it using the enthalpy values for the following individual...
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
6. Hess's Law. Use the data in Table 1 to calculate AH for the reaction below: Table 1. Change in Enthalpy for Reactions Reactions Change in Enthalpy (AH) AH = -393.5 kJ/mol (1) C() (2) Hz((g) + + O2(g) O2(g) → CO2(8) → H2O(l) AH2 = -285.8 kJ/mol (3) 2CH.(g) + 702(g) → 4 CO2(g)+ 6H2O(1) AH = -283.0 kJ/mol Calculate the enthalpy change for the reaction: 2 C(s) + 3H2(g) → CzH6(g) AH = kJ/mol
6. Hess's Law. Use the data in Table 1 to calculate AH for the reaction below: Table 1. Change in Enthalpy for Reactions Reactions Change in Enthalpy (AH) AH = -393.5 kJ/mol (1) C() (2) Hz((g) + + O2(g) O2(g) → CO2(8) → H2O(l) AH2 = -285.8 kJ/mol (3) 2CH.(g) + 702(g) → 4 CO2(g)+ 6H2O(1) AH = -283.0 kJ/mol Calculate the enthalpy change for the reaction: 2 C(s) + 3H2(g) → CzH6(g) AH = kJ/mol
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
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
Calculate the standard enthalpy change for the reaction 2C8H18(l) + 17O2(g) →16CO(g) + 18H2O(l). Given 2C8H18(I) + 25O2(g) →16CO2(g) + 18H2O(I) ΔH°=-11,020 kJ/mol 2CO(g) + O2(g) → 2CO2(g) ΔH° = -566.0 kJ/mol 0 -6,492 kJ/mol 15,550 kJ/mol 10,450 kJ/mol -10.450 kJ/mol 6,492 kJ/mol
Given the following enthalpy change values for the reactions below: A + B → 2C ; ΔH = -461.7 kJ mol-1 E + F → C + 2D ; ΔH = 279.9 kJ mol-1 ½ E + G → H ; ΔH = -203.2 kJ mol-1 Calculate ΔH for the following reaction (in kJ mol-1) using Hess's Law: A + B + 4G +4D → 4H + 2F