Answer:
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Answer:
The mass in grams of N₂O gas that can be dissolved is 0.18 g
Explanation:
The solubility of a gas is proportional to the partial pressure of that gas, over a determined solvent. That's what Henry's law states. We see the formula:
S = K . Pp
Where S is solubility and K is Henry's constant. This specific for each gas and each temperature, while Pp means partial pressure.
We replace data:
S = 0.025 M/atm . 0.69atm
S = 0.01725 M
This is the solubility of the gas, so now, we need to know what mass of gas is solubilized. We convert the moles, with the volume of water.
0.01725 mol/L . 0.235 L = 4.05×10⁻³ moles
Now, we determine the mass in grams: 4.05×10⁻³ mol . 28 g / 1mol =
0.1782 g
Answer:
we find the chemical equilibrium constant by balancing the number of reactant and products
Explanation:
and after balancing using formula (KC) = Ratio of product / reactants
Answer : The standard cell potential of the reaction is, -1.46 V
Explanation :
The given balanced cell reaction is,
Here, chromium (Cr) undergoes oxidation by loss of electrons and act as an anode. Lead (Pb) undergoes reduction by gain of electrons and thus act as cathode.
The standard values of cell potentials are:
Standard reduction potential of lead ![E^0_{[Pb^{2+}/Pb]}=-0.13V](https://tex.z-dn.net/?f=E%5E0_%7B%5BPb%5E%7B2%2B%7D%2FPb%5D%7D%3D-0.13V)
Standard reduction potential of chromium ![E^0_{[Cr^{3+}/Cr]}=1.33V](https://tex.z-dn.net/?f=E%5E0_%7B%5BCr%5E%7B3%2B%7D%2FCr%5D%7D%3D1.33V)
Now we have to calculate the standard cell potential for the following reaction.
![E^0=E^0_{[Pb^{2+}/Pb]}-E^0_{[Cr^{3+}/Cr]}](https://tex.z-dn.net/?f=E%5E0%3DE%5E0_%7B%5BPb%5E%7B2%2B%7D%2FPb%5D%7D-E%5E0_%7B%5BCr%5E%7B3%2B%7D%2FCr%5D%7D)
Therefore, the standard cell potential of the reaction is, -1.46 V
