Yes, it will be worthwhile to investigate finding a catalyst to use in this reaction under standard conditions because it is negative.
<h3>What is a Catalyst?</h3>
This is a substance which speeds up the rate of a chemical reaction by lowering the activation energy.
ΔG being negative indicates a a slow reaction which is why a catalyst under standard conditions should be used.
Read more about Catalyst here brainly.com/question/12507566
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Answer:
= -356KJ
<em>therefore, the reaction where heat is released is exothermic reaction since theΔH is negative</em>
Explanation:
given that enthalpy of gaseous reactants decreases by 162KJ and workdone is -194KJ
then,
change in enthalpy (ΔH) = -162( released energy)
work(w) = -194KJ
change in enthalpy is said to be negative if the heat is evolved during the reaction while heat change(ΔH) is said to be positive if the heat required for the reaction occurs.
At constant pressure the change in enthalpy is given as
ΔH = ΔU + PΔV
ΔU = change in energy
ΔV = change in volume
P = pressure
w = -pΔV
therefore,
ΔH = ΔU -W
to evaluate energy change we have,
ΔU =ΔH + W
ΔU = -162+ (-194KJ)
= -356KJ
<em>therefore, the reaction where heat is released is exothermic reaction since theΔH is negative</em>
Answer:
copper is being reduced
Explanation: I got 100% on the quiz good luck this class is hard lol
I’m almost sure it’s D but i could be wrong
The answer is (1) Arrhenius acid and an electrolyte. The HNO3 is a H+ ion donor and OH- receptor. Electrolyte means the compound will release ion when dissolving in suitable ionized solution.
