<h2>
1.25 g of 
would be produced from the complete reaction of 25 mL of 0.833 mol/L 
with excess 
</h2>
Explanation:
To calculate the number of moles for given molarity, we use the equation:
According to stoichiometry:
1 mole of 
will give = 1 mole of
0.0208 moles of will give =
of
Mass of 
Thus 1.25 g of would be produced from the complete reaction of 25 mL of 0.833 mol/L with excess
Learn more about molarity
https://brainly.in/question/13034158
#learnwithbrainly
Answer:
D. It predicts whether or not a reaction will be spontaneous.
Explanation:
<em>What does Gibbs free energy (ΔG) predict?
.</em>
A. It predicts what the rate of the reaction will be. NO. ΔG is a thermodynamical parameter and it is not related to the kinetics of the reaction.
B. It predicts how high the activation energy is. NO. ΔG is a thermodynamical parameter and it is not related to the kinetics of the reaction.
C. It predicts if entropy will increase or decrease. NO. ΔG depends on the entropy but not the other way around.
D. It predicts whether or not a reaction will be spontaneous. YES. If ΔG < 0 the reaction is spontaneous and if ΔG > 0 the reaction is not spontaneous.
The universe comes into existence is first
The first neutral atoms form is second
The universe begins expanding is third
Gases form that will later go to shape stars and galaxies is fourth
Atomic nuclei form is last
I'm almost certain that is correct. Do not take my word for this.
The answer would be metal
Answer:
Final concentrations:
Cu²⁺ = 0
Al³⁺ = 3.13 mmol/L = 84.51 mg/L
Cu = 4.7 mmol/L = 300 mg/L
Al = 0.57 mmol/L = 15.49 mg/L
Explanation:
2Al (s) + 3Cu²⁺ (aq) → 2Al³⁺ (aq) + 3Cu (s)
Al: 27 g/mol ∴ 100 mg = 3.7 mmol
Cu: 63.5 g/mol ∴ 300 mg = 4.7 mmol
3 mol Cu²⁺ _______ 2 mol Al
4.7 mmol Cu²⁺ _____ x
x = 3.13 mmol Al
4.7 mmol of Cu²⁺ will be consumed.
3.13 mmol of Al will be consumed.
4.7 mmol of Cu will be produced.
3.13 mmol of Al³⁺ will be produced.
0.57 mmol of Al will remain.
