Question

In: Chemistry

Consider the reaction N2(g) + 3H2(g) → 2NH3(g)ΔH o rxn = −92.6 kJ/mol If 2.0 moles...

Consider the reaction

N2(g) + 3H2(g)

2NH3(g)ΔH

o

rxn

= −92.6 kJ/mol

If 2.0 moles of N2 react with 6.0 moles of H2 to form NH3, calculate the work done (in joules) against a pressure of 1.0 atm at 25 degrees celsius.

What is ΔU for this reaction? Assume the reaction goes to completion.

Solutions

Expert Solution


Related Solutions

1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g)...
1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g) 2)Before investigating the scene, the technician must dilute the luminol solution to a concentration of 6.00×10−2M . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted spray? 3)A student placed 11.0 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve...
For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains...
For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains 0.3M N2(g) and 4.0M NH3(g). What is the concentration of H2(g)?
Ammonia can be synthesized by the reaction: 3H2(g) + N2(g) —-> 2NH3(g) What is the theoretical...
Ammonia can be synthesized by the reaction: 3H2(g) + N2(g) —-> 2NH3(g) What is the theoretical yield of ammonia, in kg, that we can synthesize from 5.43kg of H2 and 32.4 kg of N2?
1) In the balanced reaction N2(g) + 3H2 (g) -----> 2NH3 (g), what mass of ammonia...
1) In the balanced reaction N2(g) + 3H2 (g) -----> 2NH3 (g), what mass of ammonia could be produced from 7.628 grams of hydrogen gas? 2) How many lithium atoms are present in 68.7 grams of Li2O? 3) How many grams of carbon are present in 0.55 grams of acetaminophen? The formula for acetaminophen is C8H9O2N, and its molar mass is 151.18 g/mol. 4) What is the mass, in amu, of 8.441 moles of lead (ii) oxide? 5) For the...
For the production of ammonia from its elements, 3H2(g)+N2(g)→2NH3(g), ΔH = -21.9 kcal. Part A: Is...
For the production of ammonia from its elements, 3H2(g)+N2(g)→2NH3(g), ΔH = -21.9 kcal. Part A: Is this process endothermic or exothermic?    Part B: How many kilocalories are involved in the production of 27.75 g of NH3? Part C: How many kilocalories are involved if 26.90 g of H2 are consumed in this reaction?
Consider the following set of reactions: N2 + 2O2→N2O4 ,ΔH=−8 kJ/mol N2 + O2→2NO ,ΔH=180 kJ/mol...
Consider the following set of reactions: N2 + 2O2→N2O4 ,ΔH=−8 kJ/mol N2 + O2→2NO ,ΔH=180 kJ/mol The equations given in the problem introduction can be added together to give the following reaction: overall: N2O4→2NO + O2 However, one of them must be reversed, reaction 1: N2 + 2O2→N2O4 What is the enthalpy for reaction 1 reversed? reaction 1 reversed: N2O4→N2 + 2O2 Express your answer numerically in kilojoules per mole. What is the enthalpy for reaction 2?
Consider the following system at equilibrium N2(g)+3H2(g) <------> 2NH3(g)+ heat Indicatre which way the reaction wil...
Consider the following system at equilibrium N2(g)+3H2(g) <------> 2NH3(g)+ heat Indicatre which way the reaction wil shift when making the following changes 1. Decreasing in the temperture 2. Increasing in the temperture 3. Removing some of NH3 4. Removing some of the H2O 5. Adding some O2 6. Removing some N2 ****Pick from these answers **** A. Forward reaction will increase B. Reverse reaction will increase C. There will be no change in either direction
A student ran the following reaction in the laboratory at 684 K: N2(g) + 3H2(g) 2NH3(g)...
A student ran the following reaction in the laboratory at 684 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 3.26×10-2 moles of N2(g) and 6.07×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 5.83×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = __
A student ran the folllowing reaction in the laboratory at 661 K: 2NH3(g) N2(g) + 3H2(g)...
A student ran the folllowing reaction in the laboratory at 661 K: 2NH3(g) N2(g) + 3H2(g) When she introduced NH3(g) at a pressure of 0.597 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of H2(g) to be 0.879 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.
The ΔH°rxn for the following reaction is −114.2 kJ/mol. At what temperature (in °C) would the...
The ΔH°rxn for the following reaction is −114.2 kJ/mol. At what temperature (in °C) would the Kc for the reaction be 6.4 x 109? 2NO(g) + O2(g) ↔ 2NO2(g) Kc = 4.9 x 105 at 184°C 271°C 183°C 110°C 74°C
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT