1. Calculate the change in enthalpy for this reaction: 2C(s) + H2(g) → C2H2(g) Given the...
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
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...
Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ Express your answer with the appropriate units. Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ Express your answer with the appropriate units.
Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ
Calculate the enthalpy change for the reaction NO(g) + O(g) → NO2(g) from the following data NO(g) + O3(9) → NO2(g) + O2(g) ΔH=-198.9 kJ/mol O3(g) → 1.5O26(g) ΔH=-142.3 kJ/mol O2(g) → 2O(g) ΔH = 495.0 kJ/mol A. 153.8 kJ B. 190.9 kJ C.-551.6 kJ D.-304.1 kJ E. 438.4 kJ
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 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....
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the reaction: 6 C (s) + 7 H2(g) → C6H14 (l) ΔHrxn = ? C6H14 (l)+19/2O2 (g)→6CO2(g)+ 7H2O(g). ΔH=–3505.8kJ C(s) + O2 (g) → CO2(g) ΔH=–393.5kJ H2(g) + 1/2 O2(g) → H2O(g). ΔH = – 242.0 kJ
Calculate the standard reaction enthalpy for the reaction N2H4(ℓ) + H2(g) → 2 NH3(g) given N2H4(ℓ) + O2(g) → N2(g) + 2H2O(g) ∆H ◦ = −543 kJ · mol−1 2 H2(g) + O2(g) → 2 H2O(g) ∆H◦ = −484 kJ · mol−1 N2(g) + 3 H2(g) → 2 NH3(g) ∆H◦ = −92.2 kJ · mol−1 1.) −243 kJ · mol−1 2.) −59 kJ · mol−1 3.) −935 kJ · mol−1 4.) −151 kJ · mol−1 5.) −1119 kJ · mol−1
Find AHrxn for: C2H2(g) → 2C(s) + H2(g) given the following information: C2H2(g) + 5/2 O2(g) → 2002(g) + H2O (1) AH° = -1291 kJ C(s) + O2(g) + CO2(g) AH° = -391 kJ H2(g) + 1/2O2(g) + H2O(1) AH° = -280 kJ kJ