5.00 moles of N2 and 8.00 moles of H2 are placed in an empty container, the...

5.00 moles of N₂ and 8.00 moles of H₂ are placed in an empty container, the container is heated to 887 degrees Celsius, and a catalyst is added that catalyzes the rxn. of these gases to form NH₃ as the only product. At equilibrium 1.00 mole of NH₃ is found to be present. Find number of moles N₂ and moles H₂ present at equilibrium.

* I think that the concentrations of the reactants changes by 1 mole but I'm not enitrely sure if that is correct.

Expert Solution

N2 + 3 H2 <-----------------------> 2 NH3

5 8 0 ----------------------> initial

-x -3x +2x ---------------------> decomposition

5-x 8-3x 2x ---------------------------> equilibrium

equilibrium NH3 moles = 1.0

2x = 1.0

x = 0.5

equilibrium moles of N2 : 5 -x = 5 -0.5 = 4.5 mol

equilibrium moles of H2 : 8 -3x = 8 - 3 x 0.5 = 6.5 mol

queen_honey_blossom answered 1 year ago

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container...

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid 5.00-L container and they react according to the equation ? ? CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the concentration of carbon monoxide when equilibrium is reached?

In a given experiment 1.00 mole of N2 and 3.00 moles of H2 were placed in...

In a given experiment 1.00 mole of N2 and 3.00 moles of H2 were placed in a 3.00 L container. Equilibrium was established given the following reaction: N2(g) + 3H2(g) 2NH3(g) Complete the following table. Use numerical values in the Initial row and values containing the variable "x" in both the Change and Equilibrium rows. Let x = the amount of N2 needed to reach equilibrium. At equilibrium the concentration of NH3 is 0.0519 M. Determine the following quantities at...

One mole of N2 and 3 moles of H2 are placed in a flask at 397°C....

One mole of N2 and 3 moles of H2 are placed in a flask at 397°C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is found to be 0.258. The KP for the reaction is 4.31 × 10^-4

A 3 L container is filled with 12 moles of N2 at -140.6 °C. Calculate the...

A 3 L container is filled with 12 moles of N2 at -140.6 °C. Calculate the pressure using ideal gas equation, van der Waals equation, SRK equation, virial equation, and the compressibility factor chart correlation.

4.00 moles of HI are placed in an evacuated 5.00 L flask and then heated to...

4.00 moles of HI are placed in an evacuated 5.00 L flask and then heated to 800 K. The system is allowed to reach equilibrium. What will be the equilibrium concentration of each species

How many moles of H2 and N2 can be formed by the decomposition of 2.56 mol...

How many moles of H2 and N2 can be formed by the decomposition of 2.56 mol of ammonia, NH3?

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2 are placed in...

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2 are placed in a 1.50L container. N2(g) + 3H2(g) −⇀↽− 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Kc.

0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand...

0.924 moles of A (g) is placed in a 1.00 L container at 700 degrees Celsiusand a reaction occured. 38.8% of the gas A dissociated when equilibrium was established. 3 A (g) ⇌ 5 B (g) + 2 C (g). What is the value of the equilibrium constant, K, at this temperature? (Answer: K = 0.0241) **PLEASE SHOW WORK. THANKS**

How many moles of NH3 can be produced when 11.00 mol H2 react with 5.00 mol...

How many moles of NH3 can be produced when 11.00 mol H2 react with 5.00 mol N2? _________mol NH3 How many moles of each reactant are left over? Note that at least one must disappear. ______mol H2 remain _______mol N2 remain

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles...

Consider the reaction 2 NH3 (g) ? N2 (g) + 3 H2 (g). Suppose 6 moles of pure ammonia are placed in a 1.0 liter flask and allowed to reach equilibrium. If X represents the concentration (in M) of nitrogen present in the system once equilibrium is reached, which of the following will represent the concentration of ammonia in M? Show work A) 6

Question