Answer:
I would use calorimetric to determine the specific heat and I would measure the mass of a sample
Explanation:
I would use calorimetry to determine the specific heat.
I would measure the mass of a sample of the substance.
I would heat the substance to a known temperature.
I would place the heated substance into a coffee-cup calorimeter containing a known mass of water with a known initial temperature.
I would wait for the temperature to equilibrate, then calculate temperature change.
I would use the temperature change of water to determine the amount of energy absorbed.
I would use the amount of energy lost by substance, mass, and temperature change to calculate specific heat.
Answer:
Explanation:
<u>1. Calculate the iniital concentration of HI(g) introduced</u>
The initial concentration of HI(g), [HI(g)], is the number of moles per liter:
- [HI(g)] = 0.316mol/1liter = 0.316M
<u>2. Build the ICE (initial, change, equilibrium) table</u>
ICE table:
2HI(g) → H₂(g) + I₂(g)
I 0.316 0 0
C - 2x +x +x
E 0.316 - 2x x x (x = 3.12×10⁻²M)
<u>3. Find the equilibrium constant, Kc</u>
Animals contribute water mainly through breathing, perspiration and urination. ... When droplets of sweat evaporate from the surface of an animal's skin, they take a bit of the animal's body heat with them. They also turn into water vapor and enter the water cycle, just like water evaporating from plant leaves.
Answer:
pKa of the acid is 3.6
Explanation:
When a weak acid, HX, reacts with NaOH, the conjugate base, X⁻, is produced:
HX + NaOH → X⁻ + Na⁺ + H₂O
At the half neutralized solution, [HX] = [X-]
Based on Henderson-Hasselbalch equation:
pH = pKa + log [ X⁻] / [HX]
<em>Where pH is the pH of the buffer = 3.6</em>
<em>pKa is the pka of the solution</em>
<em>And as [ X⁻] = [HX], [ X⁻] / [HX] = 1</em>
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Replacing:
3.6 = pKa + log 1
3.6 = pKa + 0
<h3>pKa of the acid is 3.6</h3>
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Answer:it conduct thermal conductivity because of the heat it holds
Explanation: