Answer:
0 M.
Explanation:
Hello,
In this case, the undergoing reaction is:
![M(NO_3)_2+NaCN\leftrightarrow [M(CN)_4]^{-2}+NaNO_3](https://tex.z-dn.net/?f=M%28NO_3%29_2%2BNaCN%5Cleftrightarrow%20%5BM%28CN%29_4%5D%5E%7B-2%7D%2BNaNO_3)
Nonetheless, it only matters the reaction forming the given complex:
![M^{+2}+4CN^-\leftrightarrow [M(CN)_4]^{-2}](https://tex.z-dn.net/?f=M%5E%7B%2B2%7D%2B4CN%5E-%5Cleftrightarrow%20%5BM%28CN%29_4%5D%5E%7B-2%7D)
In such a way, the formation constant turns out:
![K_F=\frac{[[M(CN)_4]^{-2}]_{eq}}{[M^{+2}]_{eq}[CN^{-}]_{eq}^4}](https://tex.z-dn.net/?f=K_F%3D%5Cfrac%7B%5B%5BM%28CN%29_4%5D%5E%7B-2%7D%5D_%7Beq%7D%7D%7B%5BM%5E%7B%2B2%7D%5D_%7Beq%7D%5BCN%5E%7B-%7D%5D_%7Beq%7D%5E4%7D)
Now, one could assume that the initial concentrations of the ions equals the original compounds concentrations:
![[M^{+2}]_0=0.150M;[CN^-]_0=0.820M](https://tex.z-dn.net/?f=%5BM%5E%7B%2B2%7D%5D_0%3D0.150M%3B%5BCN%5E-%5D_0%3D0.820M)
In such a way, we modify the formation constant in terms of the change
due to the reaction progress:

Now, solving for
:

The feasible solution is 0.15M which will lead to an equilibrium concentration of M⁺² of 0M
![[M^{+2}]_{eq}=0.15M-0.15M=0M](https://tex.z-dn.net/?f=%5BM%5E%7B%2B2%7D%5D_%7Beq%7D%3D0.15M-0.15M%3D0M)
This fact has sense since the formation constant is very large.
Best regards.
M=147/9 x8 m=15kg
The mass of falling rock is 15kg.
Based on the data provided;
- number of moles of helium gas is 1.25 moles
- pressure at peak temperature is 259.3 kPa
- internal pressure is above 256 kPa, therefore, the balloon will burst.
- pressure should be reduced to a value less than 256 kPa by reducing the temperature
<h3>What is the ideal has equation?</h3>
The ideal gas equation relatesthe pressure, volume, moles and temperature of a gas.
The moles of helium gas is calculated using the Ideal gas equation:
n is the number of moles of gas
R is molar gas constant = 8.314 L⋅kPa/Kmol
P is pressure = 239 kPa
T is temperature = 21°C = 294 K
V is volume = 12.8 L
Therefore;
n = PV/RT
n = 239 × 12.8 / 8.314 × 294
n = 1.25 moles
The number of moles of helium gas is 1.25 moles
At peak temperature, T = 46°C = 319 K
Using P1/T1 = P2/T2
P2 = P1T2/T1
P2 = 239 × 319/294
P2 = 259.3 kPa
The pressure at peak temperature is 259.3 kPa
At 42°C, T = 315 K
Using P1/T1 = P2/T2
P2 = P1T2/T1
P2 = 239 × 315/294
P2 = 256.07 kPa
Since the internal pressure is above 256 kPa, the balloon will burst.
The pressure should be reduced to a value less than 256 kPa by reducing the temperature.
Learn more about gas ideal gas equation at: brainly.com/question/12873752
Molecular weight= 1.00784 u
mass of one mole = 1.008 grams