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24. Consider the combustion of hydrogen given below H2(g) + ½Og(g) H2O(g) ΔH =-241.8 kJ/mol →...
Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ...
Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ 2) X(s)+2Cl2(g)⟶XCl4(s)Δ?2=+157.3 kJ2) X(s)+2Cl2(g)⟶XCl4(s)ΔH2=+157.3 kJ 3) 12H2(g)+12Cl2(g)⟶HCl(g)Δ?3=−92.3 kJ3) 12H2(g)+12Cl2(g)⟶HCl(g)ΔH3=−92.3 kJ 4) X(s)+O2(g)⟶XO2(s)Δ?4=−769.5 kJ4) X(s)+O2(g)⟶XO2(s)ΔH4=−769.5 kJ 5) H2O(g)⟶H2O(l)Δ?5=−44.0 kJ5) H2O(g)⟶H2O(l)ΔH5=−44.0 kJ what is the enthalpy, Δ?,ΔH, for this reaction? XCl4(s)+2H2O(l)⟶XO2(s)+4HCl(g)
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) +...
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
Consider the following data. 2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ N2O5(g) +...
Consider the following data. 2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ N2O5(g) + H2O(l) 2 HNO3(l) ΔH = -92.0 kJ N2(g) + 3 O2(g) + H2(g) 2 HNO3O(l) ΔH = -348.2 kJ Use Hess's law to calculate ΔH for the reaction below. 2 N2O5(g) 2 N2(g) + 5 O2(g) ΔH = _____kJ
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following...
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following is true? (Select all that apply) the reaction is endothermic heat is given off by the surroundings the reaction is exothermic heat is absorbed by the system the enthalpy of the products is less than the that of the reactants
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be t...
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be t...
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH...
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...
6. Given H2(g) + 22 O2(g) → H2O(1), AH° = -286 kJ/mol, Determine the standard enthalpy...
6. Given H2(g) + 22 O2(g) → H2O(1), AH° = -286 kJ/mol, Determine the standard enthalpy change for the reaction 2H2O(l) → 2H2(g) + O2(g) (2 pt)
Given the thermochemical equation for the formation of H2O by burning H2 and O2:
Given the thermochemical equation for the formation of H2O by burning H2 and O2: H2(g) + 402 (8) → H2O (8) ΔH° = -241.8 kJ Calculate the ΔH for the following reaction: 2H2O (g) → 2 H2(g) + O2 (g)
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
6. Given H2(g) + 22 O2(g) → H2O(1), AH° = -286 kJ/mol, Determine the standard enthalpy change for the reaction 2H2O(l) → 2H2(g) + O2(g) (2 pt)
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