The amount of CO that would be required to generate 635 g of CO2 will be 404.14 g
<h3>Stoichiometric problem</h3>
First, let us get the equation of the reaction:
From the equation, we can see that the mole ratio of CO to that of CO2 is 1:1.
635 g of CO2 is to be generated.
Mole of 635 g CO2 = mass/molar mass = 635/44.01 = 14.43 moles
Thus, the equivalent mole of CO required will also be 14.43 moles.
Mass of 14.43 moles CO = moles x molar mass = 14.43 x 28.01 = 404.14 g
Hence, 404.14 g of CO will be required to produce 635 g of CO2
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The empirical formula for a compound that contains 48.6%C, 8.2% H, and 43.2% S by mass is 
.
<h3>What is the empirical formula?</h3>
An empirical formula tells us the relative ratios of different atoms in a compound.
We need to calculate the number of moles
Number of a mole of carbon =
48.6 g X (
) =4.05 mole
Number of a mole of hydrogen =
8.2g X (
) =8.14 mole
Number of moles of sulphur =
43.2g X (
) = 1.35 mole
Dividing each mole using the smallest number that is divided by 1.35 moles.
Carbon= 
=3
Oxygen= 
=6
Sulfur= 
=1
Empirical formula is
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Answer:
0.034 M is the molarity of sodium acetate needed.
Explanation:
The pH of the buffer solution is calculated by the Henderson-Hasselbalch equation:
![pH = pK_a + \log \frac{[A^-]}{[HA]}](https://tex.z-dn.net/?f=pH%20%3D%20pK_a%20%2B%20%5Clog%20%5Cfrac%7B%5BA%5E-%5D%7D%7B%5BHA%5D%7D)
Where:
pK_a= Negative logarithm of the dissociation constant of a weak acid
![[Ac^-]](https://tex.z-dn.net/?f=%5BAc%5E-%5D)
= Concentration of the conjugate base
[HA] = Concentration of the weak acid
According to the question:
The desired pH of the buffer solution = pH = 5.27
The pKa of acetic acid = 4.74
The molarity of acetic acid solution = [HAc] = 0.01 M
The molarity of acetate ion =![[Ac^-] = ?](https://tex.z-dn.net/?f=%5BAc%5E-%5D%20%3D%20%3F)
Using Henderson-Hasselbalch equation:
![5.27= 4.74 + \log \frac{[Ac^-]}{[0.01 M]}](https://tex.z-dn.net/?f=5.27%3D%204.74%20%2B%20%5Clog%20%5Cfrac%7B%5BAc%5E-%5D%7D%7B%5B0.01%20M%5D%7D)
![[Ac^-]=0.0339 M\approx 0.034M](https://tex.z-dn.net/?f=%5BAc%5E-%5D%3D0.0339%20M%5Capprox%200.034M)
Sodium acetate dissociates into sodium ions and acetate ions when dissolved in water.
![[Ac^-]=[Na^+]=[NaAc]= 0.034M](https://tex.z-dn.net/?f=%5BAc%5E-%5D%3D%5BNa%5E%2B%5D%3D%5BNaAc%5D%3D%200.034M)
0.034 M is the molarity of sodium acetate needed.
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