CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
Calculate ΔH for the reaction using the bond enthalpies given.
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
Calculate the overall enthalpy change for this reaction using the bond enthalpies given.
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
ΔH =ΔH0fproducts –ΔH0freactants
ΔH = [(ΔH0fCO2(g) )+ (2 x ΔH0fH2O (g) )]- [( ΔH0fCH4(g) )+ (2 x ΔH0fO2 (g) )]
= [ −393.5 +(2x( −241.8 ))]-[ −74.8 +(2x(0.0))]
= -802.3 kJ/mol-K
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
ΔH =ΔH0fproducts –ΔH0freactants
ΔH = [(3xΔH0fCO2(g) )+ (4 x ΔH0fH2O (g) )]- [( ΔH0fC3H8(g) )+ (5 x ΔH0fO2 (g) )]
= [ (3x(−393.5)) +(4x( −241.8 ))]-[ −103.8 +(5x(0.0))]
= -2043.9 kJ/mol-K
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) Calculate ΔH for the reaction using the...
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 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
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 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...
4. Given the reaction: CH4 (8) + 2 O2(g) → CO2 (g) + 2 H20 (8) where AH = -891 kJ Calculate the enthalpy change if 1.00 g of methane (CH) is burned in excess oxygen.
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
Calculate ΔrH for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(l) Use the following reactions and given ΔrH's. CH4(g)+O2(g)→CH2O(g)+H2O(g), ΔrH = -284 kJmol−1 CH2O(g)+O2(g)→CO2(g)+H2O(g), ΔrH = -527 kJmol−1 H2O(l)→H2O(g), ΔrH = 44.0 kJmol−1
4. In the reaction: CH4 (g) + 2 O2(g) → CO2(g) + 2 H2O(g) the initial concentration of CO2 is 0.000 M, and after 30.0 sec, the concentration of CO2 is 0.670 M. What is the average reaction rate over this time span? A) 2.50 M/s B) 0.0223 M/s C) 0.25 m/s D) 1.1 M/s
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