Question

2NH3 —> N2 (g) + 3H2 (g) If the total pressure of the gas at the...

2NH3 —> N2 (g) + 3H2 (g)

If the total pressure of the gas at the end if the reaction is 759 mmHg, calculate the partial pressures in atm of nitrogen(N2) and hydrogen (H2)

Please explain so I can understand how the answer was derived

Homework Answers

Answer #1

The given reaction is--

2NH3 ------> N2(g) + 3H2(g)

Here we can see that there is 1 mol of N2 and 3 mol of H2present.

Total number of moles = 1 + 3 = 4

Given, Ptotal = 759 mm Hg

Now, mole of N2 present / total number of moles = partial pressure of N2 / Ptotal

=> 1 / 4 = partial pressure of N2 / 759 mm Hg

=> partial pressure of N2 = 759 mm Hg / 4

=> partial pressure of N2 = 189.75 mm Hg = 189.75 mm Hg * ( 1atm /760 mm Hg) =0.249 atm

Again,

mole of H2 present / total number of moles = partial pressure of H2 / Ptotal

=> 3/ 4 = partial pressure of H2 / 759 mm Hg

=> partial pressure of H2 =( 759 mm Hg x 3) / 4

=> partial pressure of H2 = (2277 / 4) mm Hg

=> partial pressure of H2 = 569.25 mm Hg = 569.25 mm Hg *(1 atm /760 mm Hg) =0.749 atm

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Write the equation for the reaction quotient Q for a reaction. N2(g) +3H2(g)--- 2NH3(g) What is...
Write the equation for the reaction quotient Q for a reaction. N2(g) +3H2(g)--- 2NH3(g) What is the value of Q when partial pressure of nitrogen is 0.20 bar,for hydrogen 0.40 bar and for ammonium 0.61 bar?
The chemical reaction N2(g) + 3H2(g) 2NH3(g) is carried out at 400. K. Assume the partial...
The chemical reaction N2(g) + 3H2(g) 2NH3(g) is carried out at 400. K. Assume the partial pressures of N2(g), H2(g), and NH3(g) are 1.0, 4.2, and 63 atm, respectively. The value of Kp = 54 at 700. K. for this reaction. (a) Calculate the reaction free energy. (b) Indicate whether this reaction mixture is likely to form reactants, is likely to form products, or is at equilibrium.
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g)...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.7 atm N2, 3.2 atm H2, and 0.85 atm NH3 is a) -139.6 b) 0.43 c) -4.63 × 103 d) -44.1 e) -1.08 × 104
1.) The equilibrium constant for the chemical equation N2(g)+3H2(g) <--> 2NH3(g) is Kp = 1.09 at...
1.) The equilibrium constant for the chemical equation N2(g)+3H2(g) <--> 2NH3(g) is Kp = 1.09 at 209 °C. Calculate the value of the Kc for the reaction at 209 °C. 2.) At a certain temperature, 0.3411 mol of N2 and 1.581 mol of H2 are placed in a 1.50-L container. N2(g)+3H2(g) <--> 2NH3(g) At equilibrium, 0.1801 mol of N2 is present. Calculate the equilibrium constant, Kc. 3.) At a certain temperature, the Kp for the decomposition of H2S is 0.748....
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How...
Consider the following balanced reaction between hydrogen and nitrogen to form ammonia: 3H2(g) + N2(g)→2NH3(g) How many moles of NH3 can be produced from 24.0 mol of H2 and excess N2? Express the number of moles to three significant figures.
N2(g) + 3H2(g) -> 2NH3 (g) You charge a reaction vessel with 1.00 atm of all...
N2(g) + 3H2(g) -> 2NH3 (g) You charge a reaction vessel with 1.00 atm of all three gasses (N2,H2, and NH3) and allow them to come to equilibrium at 287K. you determine that 13.20% of the N2 gas has been consumed. what is delta G standard for this reaction based on these conditions?
N2(g) + 3H2(g) →2NH3(g) If there is 10.02 g N2 and excess H2 present, the reaction...
N2(g) + 3H2(g) →2NH3(g) If there is 10.02 g N2 and excess H2 present, the reaction yields 9.47 g NH3. Calculate the percent yield for the reaction
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g)...
part a The reaction of nitrogen and hydrogen to produce ammonia: N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kc= 1.2 at 375 °C. If the starting concentrations are [H2] = 0.76 M, [N2] = 0.60 M, and [NH3] = 0.48 M, at equilibrium which gases will have increased in concentration and which will have decreased in concentration? a. H2 b. N2 c. NH3 part b When solid sodium bicarbonate is heated the following decomposition reaction occurs: 2NaHCO3(s) ⇌...
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many...
N2(g) + 3H2(g) → 2NH3(g) 5.00 g N2 is reacted with 5.00 g H2 How many mol NH3 can be produced in this reaction?
Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) → 2NH3(g) Suppose that...
Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) → 2NH3(g) Suppose that at a particular moment during the reaction, molecular hydrogen is reacting at the rate of −0.091 M/s. (a) At what rate is ammonia being formed? (b) At what rate is molecular nitrogen reacting? PLEASE HELP! THANKS!