What is the value of ΔH in kJ for the overall reaction: 4 NO + 6 H2O → 4 NH3 + 5 O2
given these reaction steps?
I. N2 + O2 → 2 NO ΔH = (1.99x10^2) kJ
II. 2 NH3 → N2 + 3 H2 ΔH = (8.910x10^1) kJ
III. 2 H2O → 2 H2 + O2 ΔH = (4.8000x10^2) kJ
Please show work
Question 4 (2 points) What is the value of AH in kJ for the overall reaction: 4 NO + 6 H20 + 4 NH3 +5 O2 given these reaction steps? 1. N2 + O2 + 2 NO AH = (1.97x10^2) kJ II. 2 NH3 + N2 + 3 H2 AH = (8.870x10^1) kJ III. 2 H2O → 2 H2 + O2 AH = (4.7900x10^2) kJ Enter your answer in scientific notation with 3 sig figs. Do not include any units...
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(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 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
3. Determine the change in enthalpy for the oxidation of ammonia as follows 4 NH (g)5 O2(g) 3 4 NO(g) + 6 H2O( using the following information: I. N2(g3 H2(g)2 NH3(g) AH-99.22 kJ II. N2(gO2(g) 2 NO(g) AH0 180.5 kJ Ш. )> 2 H20(I) AH= - 571.6 kJ 2 H2(g) Ausaassskl
Show all work and calculations. Find the ΔH for the target reaction below, given the following step reactions and subsequent ΔH values: N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g) 2NH3(g) → N2H4(l) + H2(g) ΔH = 22.5 kJ 2NH3(g) → N2(g) + 3H 2(g) ΔH = 57.5 kJ CH2O(g) + H2(g) → CH 4O(l) ΔH = 81.2 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
1) State what is the net reaction.
2) What is the value for ΔH° for the net reaction?
(kJ)
Consider the following thermochemical equations: (1) CH2OH() + O2(g) HCHO2(/) + H2O(1) AH°= -411 kJ (2) CO(g) + 2H2(g) –CH2OH() AH°=-128 kJ (3) HCHO2(1) CO(g) + H2O(1) AH°= -33 kJ Suppose Equation (1) is reversed and divided by 2; Equations (2) and (3) are multiplied by V2, and then the three adjusted equations are added.
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....