Answer:
4. The reaction is spontaneous at any temperatures if the standard entropy of reaction is positive.
Explanation:
Equilibrium constant decreases on increasing the temperature . So the reaction appears to be exothermic . In other words
ΔH is negative .
Δ G = ΔH - TΔS
If ΔS is positive , second term is negative . ΔH is negative so the RHS of the equation is negative at all temperatures . Hence Δ G of the reaction is negative . So reaction is spontaneous at any temperature.
To solve this equation you can use a basic molarity formula and substitute the correct values.
The formula for molarity is M = mol/L.
Start by changing your mL to L. To do this, divide 25 by 1000.
This results in:
.025 L
You can now rearrange your molarity formula to isolate what you are solving for, which is moles.
This leaves your formula as:
ML = mol
Now, plug in your converted volume and given molarity into the formula.
This leaves you with:
(0.100)(0.025) = mol
Multiply to find your final value for moles.
This results in:
0.0025 mol of HNO3
I hope this is what you’re looking for! :)
C. The salt bridge maintains the flows of ions and allows electrons to move from the anode to the cathode.
i think its a right tringle
