Explanation:
The equation is given as;
N2O(g) ⇄ N2(g) + O(g)
k₁ = Forward reaction
k₋₁ = Reverse Reaction
Equilibrium concentration (K) = k₁ / k₋₁
![K = \frac{[N2O] }{[N2] [ O]}](https://tex.z-dn.net/?f=K%20%3D%20%5Cfrac%7B%5BN2O%5D%20%7D%7B%5BN2%5D%20%5B%20O%5D%7D)
Answer is: the solubility of silver oxalate is <span>a. 1.4 × 10-4 m.
</span>
<span>Chemical reaction
(dissociation) of silver oxalate in water:
Ag</span>₂C₂O₄(s) → 2Ag⁺(aq) + C₂O₄²⁻<span>(aq).
Ksp(Ag</span>₂C₂O₄) = [Ag⁺]²·[C₂O₄²⁻<span>].
[C</span>₂O₄²⁻] = x; solubility of oxalate ion.
[Ag⁺] = 2[C₂O₄²⁻<span>] = 2x
1.0·10</span>⁻¹¹ = (2x)² · x = 4x³.
x = ∛1.0·10⁻¹¹ ÷ 4.
x = 1.4·10⁻⁴ M.
Explanation:
At 365 K temperature sulfur tetrafluoride have a density of 0.260 g/L at 0.0721 atm.
What is an ideal gas equation?
The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
First, calculate the moles of the gas using the gas law,
PV=nRT, where n is the moles and R is the gas constant. Then divide
the given mass by the number of moles to get molar mass.
Given data:
P= 0.0721 atm
n=\frac{mass}{molar \;mass}n=
molarmass
mass
R= 0.082057338 \;L \;atm \;K^{-1}mol^{-1}R=0.082057338LatmK
−1
mol
−1
T=?
Putting value in the given equation:
\frac{PV}{RT}=n
RT
PV
=n
density = \frac{2 \;atm\; X molar\; mass}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X T}density=
0.082057338LatmK
−1
mol
−1
XT
2atmXmolarmass
0.260 g/L = \frac{0.0721 \;atm\; X 108.07 g/mol}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X T}0.260g/L=
0.082057338LatmK
−1
mol
−1
XT
0.0721atmX108.07g/mol
T = 365.2158727 K= 365 K
Hence , at 365 K temperature sulfur tetrafluoride have a density of 0.260 g/L at 0.0721 atm.
