Q = mCΔT
Q is heat in Joules, m is mass, C is the specific heat of water, delta T is the change in temperature
Q = (35g)(4.18)(35 degrees) = 5121 Joules or 5.12 kJ required
Explanation:
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Answer:
Mole fraction of Nacl is 0.173
Explanation:
we know that
![P_{sol}=\chi_{solvent}P^0_{solvent}](https://tex.z-dn.net/?f=P_%7Bsol%7D%3D%5Cchi_%7Bsolvent%7DP%5E0_%7Bsolvent%7D)
where,
P
sol - the vapor pressure of the solution
χ solvent - the mole fraction of the solvent
P
∘
solvent - the vapor pressure of the pure solvent
This means that in order to be able to calculate the mole fraction of sodium chloride, you need to know what the vapor pressure of pure water is at
25
°
C You can use an online calculator to find that the vapor pressure of pure water at 25 C is equal to about 23.8 torr
.
![\chi_{water}= \frac{P{sol}}{P^0{water}}](https://tex.z-dn.net/?f=%5Cchi_%7Bwater%7D%3D%20%5Cfrac%7BP%7Bsol%7D%7D%7BP%5E0%7Bwater%7D%7D)
=0.827
Also we know that
![\chi_{water}+\chi_{Nacl}= 1](https://tex.z-dn.net/?f=%5Cchi_%7Bwater%7D%2B%5Cchi_%7BNacl%7D%3D%201)
This means that the mole fraction of sodium chloride is
χ_{Nacl}= 1-Χ_{water}
= 1-0.827 =0.173
Answer:
The answer to your question is 1 M
Explanation:
Data
Molarity = ?
mass of CaCl₂ = 222.2 g
Volume = 2 l
Process
1.- Calculate the molar mass of CaCl₂
CaCl₂ = 40 + (35.5 x 2) = 40 + 71 = 111 g
2.- Calculate the moles of CaCl₂
111g of CaCl₂ ---------------- 1 mol
222.2 f of CaCl₂ ---------------- x
x = (222.2 x 1) / 111
x = 222.2 / 111
x = 2 moles
3.- Calculate the Molarity
Molarity = moles / Volume
-Substitution
Molarity = 2/2
-Result
Molarity = 1
Answer: The standard free energy change for a reaction in an electrolytic cell is always positive.
Explanation:
Electrolytic cells use electric currents to drive a non-spontaneous reaction forward.
Relation of standard free energy change and emf of cell
![\Delta G^o=-nFE^0_{cell}](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo%3D-nFE%5E0_%7Bcell%7D)
where,
= standard free energy change
n= no of electrons gained or lost
F= faraday's constant
= standard emf
= standard emf = -ve , for non spontaneous reaction
Thus ![\Delta G^o=(-ve)(-ve)=+ve](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo%3D%28-ve%29%28-ve%29%3D%2Bve)
Thus standard free energy change for a reaction in an electrolytic cell is always positive.