N2(g) + 3H2 (g) // 2NH3 (g) Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 4.51 × 10⁻⁶ at a particular temperature. Calculate the value of Qp for the initial set reaction conditions: 57 atm NH₃, 27 atm N₂, 82 atm H₂. (35)
Showtranscribed image text Consider the following reaction: N2(g) + 3 H2(g) 2NH3(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Assume that all concentrations are equilibrium concentrations in M.
Clickhere👆to get an answer to your question ️ 61. N2(g) +3H2(g) 2NH3(g) For the reaction initially the mole ratio was 1 : 3 of N2 : H2. At equilibrium 50% reacted. If the equilibrium pressure is P the partial pressure of NH3 at equilibrium is: of each has 3 6 8
Enla reacción química N2 + 3H2 → 2NH3, la velocidad de reacción del hidrógeno es de 0,084 M/s. Como la reacción es una reacción redox, la velocidad de reacción del amoniaco es la mitad de la velocidad de reacción del hidrógeno, que es de 0,042 M/s. La velocidad de reacción del nitrógeno es también de 0,042 M/s. N2(g) + 3H2(g) →
一定温度下反应N2g）+3H2（g）⇌2NH3（g）达到化学平衡状态的标志是（ ） A.单位时间里每增加1molN2，同时减少2molNH3 B.c（N2）：c（H2）：c（NH3）=1：3：2 C.N2与H2的物质的量与NH3的物质的
反应N2g)+3H2(g) 2NH3(g)ΔrHmө=-92kJ·mol-1，从热力学观点看要使H2达到最大转化率，反应的条件应该是 A．低温高压 B．低温低压
WCa3. >>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
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.
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
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
n2 g 3h2 g 2nh3 g
