Transcribed image text N2 g+3H2 g→2NH3 g Consider a reaction between a L flask containing nitrogen gas and a L flask of hydrogen gas. Both gases have a temperature of 305 K and the pressures inside both flasks is bar. What mass of ammonia in g would you expect to be produced at temperature 305 K and a pressure of bar?Previous question Next questionThis problem has been solved!You'll get a detailed solution from a subject matter expert that helps you learn core Answer
Forthe reaction N2(g) + 3H2(g) = 2NH3(g), K = 1.60 x 10-4 at 400 °C. Calculate (a) ~rGo and (b) ~rG when the pressures of N2 and H2 are maintained at 10 and 30 bar, respectively, and NH3 is removed at a partial pressure of 3 bar. (c) Is the reaction spontaneous under You first need to solve for the moles of N2. This is done by dividing the mass given by the molar mass of N2. The molar mass is calculated by adding the molar mass of all the atoms N * 2 = N2Using as the molar mass of N2 perform the following / = N2Because the equation in balanced we already know that there are two moles of ammonia produced for every one mole of N2. This means we just need to multiply the number of moles of N2 by 2 in order to get the number of moles of ammonia N2 * 2mol NH3/1mol N2 = NH3After solving for the moles of ammonia, we need to convert the moles to grams. This is done using the molar mass of ammonia which is solved as N2 + 3 H = NH3The moles of ammonia we found earlier is then multiplied by the molar mass of ammonia to convert it to NH3 * NH3 = NH3Therefore, your answer should be of ammonia are produced. Elementalcomposition of N2(g)3H2(g)2NH3(g) Element Symbol Atomic weight Atoms Mass percent; Nitrogen: N: 14.0067: 24: 93.0267: Hydrogen: H: 1.00794: 25: 6.9733: Mass percent composition Atomic percent composition; Formula in Hill system is H25N24: Computing molar mass (molar weight) 403 ERROR The Amazon CloudFront distribution is configured to block access from your country. We can't connect to the server for this app or website at this time. There might be too much traffic or a configuration error. Try again later, or contact the app or website owner. If you provide content to customers through CloudFront, you can find steps to troubleshoot and help prevent this error by reviewing the CloudFront documentation. Generated by cloudfront CloudFront Request ID B2NgdjPlc7GqpfwFvObT9ywQaUmokz5nVM2V9QQIGwtCQdkKuKdqYQ== Forreaction N2 + 3H2 = 2NH3. 6 moles of H2 is taken with excess of N2, what is the mass of ammonia gas produced? If the reaction is considered to be irreversible, then as Azmat has calculated 4 mole of NH3 , i.e., 68 g ( not 68 u) of it will be formed. >>Class 11>>Chemistry>>Equilibrium>>Applications of Equilibrium Constants>>N2 g + 3H2 g 2NH3 g for the reacOpen in AppUpdated on 2022-09-05SolutionVerified by TopprGiven that initially, the mole ratio was of . Since, of the metal has reacted,Total no. of moles reacted No. of moles of at equillibrium Equillibrium pressure Partial pressure of at equillibrium Solve any question of Equilibrium with-Was this answer helpful? 00Similar questionsMore From ChapterLearn with Videos Practice more questions Diketahuireaksi N2 (g) + 3H2 (g) --> 2NH3 (g) jika direaksikan 5 liter gas nitrogen, maka volume gas NH3 yang terbentuk adalah 10 liter. Pembahasan : Gay-Lussac menyatakan bahwa "Perbandingan volume gas yang bereaksi dan hasil reaksi pada suhu dan tekanan yang sama akan sebanding dengan koefisien reaksinya." Transcribed image text 1. Write the equilibrium expression for the following reaction 2 points N2 g + 3H2 g 2NH3g 2. Calculate the equilibrium constant for the reaction below using the balanced chemical equation and the concentrations of the substances at equilibrium. 2 points N2g + 3H2g 2NH3 8 [N2] - M [H2] = M NH3 - M 3. Are reactants or products favored at equilibrium? 2 points 4. Calculate the equilibrium constant for the reaction below using the balanced chemical equation and the concentrations of the substances at equilibrium. 2 points N2 g + 3H2g 2NH3g [N2] M [H2] M NH3 - M 5. Compare your answers to Problems 2 & 4. Are your solutions to Problem 2 & 4 in agreement? 1 point Make a statement regarding the equilibrium constants you determined and the concentrations of substances at equilibrium. 1 point 5. Compare your answers to Problems 2 & 4. Are your solutions to Problem 2 & 4 in agreement? 1 point Make a statement regarding the equilibrium constants you determined and the concentrations of substances at equilibrium. 1 point Previous question Next question 2NH3的体积是（A）A.（V1V2V3）L B.（V1V2V3）L C.（V1V22V3）L D.V3（V1V2） L【解析】 N2 3H2 2NH3 V 1 3 2 2（V1V2V3）L根据比例即可得到答案。 （）C3H83H2O 3CO 7H2， COH2O=CO2H21mol 3mol 7mol 3mol 3mol1mol C3H8可生成10mol H2N2 3H2 2NH3 3 2 10mol (6.7mol)【题4】把氮气和氢气按：的物质的量比对于容积不变密闭容器中的反应N2（g）+3H2（g）⇌2NH3（g）； H＜0，在673K，30MPa下n（NH3）和n（H2）随时间变化的关系如图所示．下列叙述不正确的是（ ）nae NH3bcdH20t t2t A. 点a处的正反应速率比点b处的大 B. 点c处的正反应速率与逆反应速率相等 C. 点d（t1时刻）的n（N2）比点e（t2时刻）处的n（N2）大 D
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N2g) + 3H2(g) — 2NH3(g) (g tepkimesi için N, nin ortalama harcanma hızı 2.10-3 dır. -3 mol Ls Bu tepkime i > Soru çözme uygulaması ile soru sor, cevaplansın. KAYDOL GİRİŞ YAP Dersler
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Equilibriumconstant, Kc for the reaction N2(g) + 3H2 (g) ----- 2NH3 (g) at 500 K is 0.061 At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L-' N„ 2.0 mol L-' H2 and 0.5 mol L-' NH3. Is the
Explanation The reaction: N2 (g) + 3H2 (g) → 2NH3 (g) 20 ml of Nitrogen given. So, 1 volume of nitrogen gas reacts with 3 volumes of hydrogen gas to produce 2 volumes of ammonia gas. For this gaseous reaction in which all the reactants and products are gases we could write a chemical equation: 1 volume N2 (g) + 3 volumes H2 (g) → 2 volumes
GivenN2(g) + 3H2(g) 2NH3(g), increasing the pressure will cause more NH3 to form. According to LeChatelier's Principle, an increase in pressure moves the equilibrium in the direction where
Theequilibrium constant, Kc, for the following reaction is 1.05 at 653 K. 2NH3(g) N2(g) + 3H2(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 653 K, the equilibrium concentration of H2(g) is found to be 0.429 M. Calculate the concentration of NH3 in the equilibrium mixture.
Showyour answers clearly for all the following questions 1. Using the conservation of mass law. predict the mass of Nigas produced from the reaction of 1.000 g N2 and 0.216 g Hz. 00 Nag) + 3H2(g) + 2 NH ) 1.216 8NH, 1 0.91 2.
