Solution of problem shown in the following Image
. For the reaction C(s)+O2(g) CO2(g), AH = -393.5 kJ/mol. What is the amount of heat...
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...
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
[32] The enthalpy of reaction for [6] enthalpy of reaction for the combustion of C to CO, is-393.5 kJ/mol C, and the enthalpy for the combustion of CO to CO, is-283.0 kJ/mol CO: (i) C(s) + O2(g) + CO2(e) AH -393.5 kJ CO(g) + O2(g) + CO2(g) AH -283.0 kJ Using these data, calculate the enthalpy for the combustion of C to CO. (iii) C(s) + O2(g) - CO(g) AH-?
Given the following equations and AH' values: C(s) + O2(g) + CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) - H20 (1) AH = -285.8 kJ 2C2H2 (8) + 5O2(g) + 4CO2(g) + 2H20 (1) AH'= -2598 kJ Determine the heat of reaction (in kJ) at 298 K for the reaction: 2C(s) + H2(8) C2H2 (8) 0-136.8 0-219.8 0-109.9 O-167.1 +226.2
en 18 What is AH of the following reaction? CO2(g) + 2CH2(g) → C3H5(g) + O2(g) Substance AH,(kJ/mol) CO2(g) -393.5 out of -74.9 CH4(g) CH3(g) -104.7 Select one: a. -573.1 kJ O b. 348.4 kJ O a. 438.6 kJ O d. -648.0 kJ -348.4 kJ
Coal burns in oxygen exothermically as shown below: C(s) + O2(g) → CO2 (g) AH = -393.5 kJ What amount of heat will be released when 100.0 g of it is burned? Molar mass of C = 12.01/mol -3935 kJ -0.3930 kJ -3276 kJ -4726 kJ
C(s) + O2(g) + CO2(g) AH° = -393.5 kJ (5 pts) Given the following enthalpy values for reactions at 25°C, what is AH at 25°C for the following reaction: C3H3(g) + 502(g) + 4H2O(g) + 3CO2(g) AH = -2043 kJ 3C(s) + 4 H2(g) → C3H8 (g) 2H2(g) + O2(g) + 2H2O(g) AH° = -483.6 kJ
Calculate the heat change, in kJ, if 8.7395x1012 ng of carbon dioxide were produced in the following reaction: C(s) + O2(g) CO2(g) AH = -393.5 kJ/mol q=C MAT
From the following data, C(graphite) + O2(g) → CO2(g) AHrxn = -393.5 kJ/mol H2(g) + O2(g) → H200) AH"rxn = -285.8 kJ/mol 2C2H6(g) + 702(g) -> 4CO2(g) + 6H2O(l) Arxn=-3119.6 kJ/mol Calculate the enthalpy change for the reaction: 2 C(graphite) + 3H2(g) + C2H668)
1. Given AH (CO2(g)) - -393.5 kJ/mole, AH (CH2(g)) = -146.4 kJ/mole HO )) - -241.8/mote and AH (a) (10 points) How much heat is evolved if 36.0 g CsHis undergoes combustion at constant pressure? (b) (10 points) What volume of O2(g) is required in the combustion at 25°C and 1.00 atm if 9,818 kJ are evolved?