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3. Consider the reaction between nitrogen and oxygen to form dinitrogen monoxide: 2 N2(g) + O2(g)...
Consider the reaction between nitrogen and oxygen gas to form dinitrogen monoxide: 2N2(g)+O2(g)→2N2O(g),ΔHrxn=+163.2kJ Part A Calculate the entropy change in the surroundings associated with this reaction occurring at 25∘C. Express the entropy change to three significant figures and include the appropriate units.
Nitrogen monoxide (NO) reacts with oxygen (O2) to form nitrogen dioxide (NO2): NO(g) + O2(g) → NO2(g) Initial rates for the reaction of nitrogen monoxide (NO) and oxygen (02) were measured at 25°C starting with various concentrations of NO and O2. The following data were collected: Exp. [NO]. (A) [02]. (A) d[NO]/dt (M/s) 0.020 0.010 -0.056 0.020 0.020 -0.112 3 0 .020 0.040 -0.224 0.040 0.020 -0.448 5 0.010 0.020 -0.028 4 What is the numerical value of the rate...
When nitrogen gas is combined with oxygen gas to form nitrogen monoxide, according to the reaction N2 + O2 → 2NO, what can be used to measure the rate of the reaction? Group of answer choices: A) N2 consumption B) NO formation C) Both A and B D) O2 production
Question 16 5 pts The thermochemical equation for the reaction of oxygen and nitrogen monoxide to form nitrogen dioxide is 2NO(g) + O2(g) 2NO2(g) AH = -114 kJ What is AH for the reaction re-written in the form NO2(g) -> NO(g) + KO2(g) AH = ? 228 kJ 114 kJ -57 kJ - 114 kJ 57 kJ
Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10 g dinitrogen monoxide decomposes? (Be sure to write a balanced equation. You are given the reactants and products) a.) 0275 g b.) 3.64 g c.) 7.27 g d.) 14.5 g
The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) 2NO(g) At 2000°C, the equilibrium constant, Kc, has a value 7.75, what is the value of Kp? Select one: A. 4.10 × 10–4 B. 2.17 × 10–8 C. 7.75 D. 7.65 × 10–2 E. None of these choices are correct.
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
7. Nitrogen dioxide is formed from nitrogen monoxide and oxygen in a product favored reaction at 25°C. Determine the standard entropy change AS, for the reaction AS9rxn (=AS sys). AS for NO2 is 240.1 JK' mol!. As for NO is 210.8 JK 'mol!, AS for O2 is 205.1 J K mol'. Remember to scale each entropy value by the number of moles of reactant or product involved.
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) + N2O(g) --> N2(g) + NO2(g) (slow) 2 NO2(g) --> 2 NO(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [N2O]2 Rate = k [NO] [NO2] Rate = k [N2O]2 [N2O] Rate = k [NO2] [N2O] Rate = k [N2O] [N2O] Rate = k [NO] [N2O] (b) Choose...