Answer: 0.0508mL
Explanation: Using the basic formula that states: C acid * V acid = C base * V base. we have:0.568 * 17.88 = 20 * C base.
therefore concentration of the base is 1.0156/20 = 0.0508 mL
Pressure = (weight) / (area supporting the weight).
From the fraction, you can see that <em>more weight </em>produces more pressure,
and <em>less area</em> produces more pressure.
So, for the greatest pressure, you want the greatest weight supported by
the smallest area.
That would be the 55-kg boy, standing on one foot.
For the answer to the answer above, the excess energy must be absorbed to overcome the lattice energy, and then energy is released as the ions are hydrated.
So, the heat of solution =is+7.3X10^2 kJ/mol - 793 kJ/mol =
So the answer is
-63 kJ/mol
I hope you find my answer helpful.
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Answer:
a. What makes this an oxidation-reduction reaction? (1 point)
Loss of electron by the aluminum and the gain of electron by the silver
b. Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reaction. (3 points)
oxidation half reaction: Al → Al3+ + 3e-
Reduction half reaction: Ag+ + e- → Ag
c. What is oxidized in the reaction? What is reduced? (2 points)
Aluminum is oxidized and silver is reduced
d. In this simple electrochemical cell, what functions as the anode? What is the cathode? (3 points)
In a simple electrochemical cell the electrode where oxidation takes place is the anode. And the electrode where reduction reaction happens is the cathode.
e. Is this a galvanic cell or electrolytic cell? Explain your answer. (2 points)
An electrolytic cell because the reaction converts electrical energy into chemical energy
Not sure about e and f!
Answer:
0.02 m
Explanation:
∆U = q + w
w = ∆U - q = (1380 - 2040) J = -660 J
w = -p∆V = -pA∆h
∆h = -w/(pA)
p = 1 bar × (100000 Pa/1 bar) = 100000 Pa
∆h = -(-660 J)/(100000 Pa×0.33 m²) = 0.02 m
