Proposed chemical reactions I. 30, (g) → 20, (g) II. N, (g) + O2(g) → 2NO...
Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2 (g) -> 2NO2 (g), ΔHrxn = -114.1 kJ/mol 4NO2(g) + O2 (g) -> 2N2O5 (g), ΔHrxn = -110.2 kJ/mol N2 (g) + O2 (g) -> 2 NO (g), ΔHrxn = +180.5 kJ/mol
For which of the following reactions is AS™ > 0. Choose all that apply 2NO(g) + 2H2(g) + N2(g) + 2H2O(1) H2(g) + C2H4(9) + CH (9) D NHI(s)+ NH4(g) + HI(g) 2002(g) + N2(g) 2CO(g) + 2NO(g) 4NH3(9) +502(9)→ 4NO(g) + 6H20(g) Submit Answer Retry Entire Group 3 more group attempts remaining Which of the following transformations represent an increase in the entropy of the system. Choose all that apply 44 g Ag (liquid, 1.234x10°K) 44 g Ag (solid,...
Calculate ΔG0 for the following reactions at 25oC. (a) N2(g) + O2(g) → 2NO(g) ΔG0 = kJ/mol (b) H2O(l) → H2O(g) ΔG0 = kJ/mol (c) 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ΔG0 = kJ/mol
6. Given the following thermochemical reactions 2NO N,+O 2NO+O,2NO AH=-180 kJ AH=-112 kJ Calculate the enthalpy change of the reaction of nitrogen with oxygen to produce nitrogen dioxide. N,+20,2NO, AH r? Lo Given the following standard enthalpy of formations: AHor [C2H$OH(I) =-277.7 kJ/mol]; AHOr [CHCO2H) =-484.5 kJ/mol]; AHr [H2O) = -285.8 kJ/mol]; AHn[O2(g) = 0 kJ/mol]. Calculate the AHn for the reaction. C,H.OH()+O,(g) ->CH,CO,H() + H2O(1)
In the chemical equation, 2CO(g) + O2(9) > 2C02(g), the CO is a(n) product (B) reactant solid (D) element (E) none of the above
13. Given the data N,(g) + 0.9-2N0(g) 2N0(g) + O2(g) → 2NO2(g) 2N20(g)-> 2 N2(g) + O2(g) M,-+190.4 kJ/mol AH-=-129.3 kJ/mol A, =-58.7 kJ/mol For the "mol" of the units above, it means that the reaction coefficients are counted iin numbers of moles. Use Hess's law to calculate AH in kJ/mol for the reaction N20(g) + N2 (g) + 20, → 3N0(g) + NO2(g) 14. Compare the following two unbalanced violent chemical reactions that could be used in rocket engines:...
Consider following chemical reactions: 1) CHa(g) +202(8)-CO2(g) 2H20() 2) C(s) O2(g) CO2(g) 3) 2C(s)O2(g) 2CO(g) 4) 3C(s) 2H20()CH4(g)2CO(g) H2O(I) indicates that H2O is in liquid state. If the Enthalpy of reaction for reaction 1, 2, and 3 are -890.4kj, -393.5kj and -221.0kj respectively; try to figure out the Enthalpy of reaction for reaction 4. Please show your work.
The commercial production of nitric acid involves the following chemical reactions: (a) 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)⟶2NO2(g) (c) 3NO2(g)+H2O(l)⟶2HNO3(aq)+NO(g) How many grams of ammonia must you start with to make 800.00 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.
please do all
Part A Determine AG for the following reaction: 2NO(g) + O2(g)–N,04(9) Use the following reactions with known A Grxu values. N,O.(g)-2NO(9). AGRX = 2.8 kJ NO(9)+02 (9) NO2(g), AGpx = - 36,3 kJ Express your answer using one decimal place. VACAO 2 ? AGE Submit Request Answer Part A Calculate A Gin for the following reaction: 4CO (9) + 2NO2(9) 4CO2 (9) + N2 (9) Use the following reactions and given AG x values: 2NO(g) + O2(g)...
1. Which of the following is true for a chemical reaction at equilibrium? only the forward reaction stops only the reverse reaction stops both the forward and reverse reactions stop the rate constants for the forward and reverse reactions are equal the rates of the forward and reverse reactions are equal 2. A chemical equilibrium may be established by starting a reaction with reactants only. d. any quantities of reactants and products. products only. e. all the above equal quantities...