For a particular reaction, ΔH∘=67.7 kJ/mol and ΔS∘=126.9 J/(mol⋅K). Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction?T= K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature?greater thanless than

When T > 533.5K, the reaction is spontaneous in the forward reaction.

When T < 533.5K, the reaction is nonspontaneous

Explanation:

Using the equation:

ΔG = ΔH - TΔS

Where T is absolute temperature

The ΔG < 0 indicates nonspontaneus reaction, ΔG > 0 indicates spontaneous reaction.

That means:

0J/mol = 67700J/mol - T*126.9J/molK

T*126.9J/molK = 67700J/mol

T = 533.5 K

That means:

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:

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .