Consider the dehydrogenation of ethane to form ethene (ethylene) and hydrogen, latex: \text{c}_2\text{h}_6\rightleftharpo ons\text{c}_2\text{h}_4+\text{h}_2c 2 h 6 ⇌ c 2 h 4 + h 2 the standard enthalpies of formation and the standard entropies at 25 °c and 1 atm are given below, as pulled from oxtoby, gillis, and nachtrieb, principles of modern chemistry, fourth edition; fort worth: saunders, 1999. substance latex: \delta h^\circ_fδ h f ∘ (kj/mol) latex: s^\circs ∘ (j/mol/k) carbon (s, graphite) 5.74 hydrogen (g) 130.57 ethylene (g) 52.26 219.45 ethane (g) −84.68 229.49 assuming your goal is the production of hydrogen and/or ethylene, would it be beneficial to carry out this reaction at high pressure or low pressure, assuming kinetics are not an issue (i. e., that equilibrium is achieved reasonably quickly at any pressure)?

It would be better to carry out the reaction at low pressure

Explanation:

[\tex]C_2H_6 (g)\rightleftharpoons C_2H_4 (g)+H_2 (g)[/tex]

Assuming that the reaction above is in equilibrium and getting based on the principles of Le Chatellier we can say that:

If we increase the pressure in the system, the reaction will go Leftward because it will try to reduce the pressure by consuming moles of gas.

If we reduce the pressure in the system, the reaction will go rightward because it will try to increase the pressure by producing moles of gas.

Given that our goal is to produce ehtylene, we want the reaction to go rightward and to do so is better to work at low pressure.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: