The reaction between Ag2CO3 and NaOH is shown by the equation below
Ag2CO3 + NaOH = Ag2O + Na2CO3 +H2O
we can determine the number of mole of sodium hydroxide
by (2.85 ml × 1) ÷ 1000 ml , since according to molarity 1 mole is contained in 100ml.
we get 0.00285 moles of NaOH
Using the mole ratio we can get the moles of Ag2CO3
Mole ratio: Ag2NO3 : NaOH = 1:1
Therefore, the moles of Ag2CO3 will be 0.00285 moles
but 1 mole of silver carbonate is equivalent to 275.8 g
Thus the mass will be calculated by 0.00285 moles × 275.8g = 0.78603g
Mass of silver carbonate required will be 0.78603g
Answer:
Mass = 53.45 g
Explanation:
Given data:
Mass of propane = 200 g
Mass of S₂ = 75 g
Theoretical yield /Mass of CS₂ = ?
Solution:
Balanced Chemical equation:
C₃H₈ + 5S₂ → 4H₂S + 3CS₂
Number of moles of propane:
Number of moles = mass / molar mass
Number of moles = 200 g/ 44.1 g/mol
Number of moles = 4.54 mol
Number of moles of S₂:
Number of moles = mass / molar mass
Number of moles = 75 g/ 64.14 g/mol
Number of moles = 1.17 mol
Now we will compare the moles of carbon disulfide with both reactant.
S₂ : CS₂
5 : 3
1.17 : 3/5×1.17 = 0.702
C₃H₈ : CS₂
1 : 3
4.54 : 3×4.54 = 13.62 mol
Number of moles of CS₂ produced by S₂ are less so it will limiting reactant and limit the yield of carbon disulfide.
Theoretical yield of carbon disulfide.
Mass = number of moles ×molar mass
Mass = 0.702 mol × 76.14 g/mol
Mass = 53.45 g
Answer:
The answer to the question is
The equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains 0.26 atm.
Explanation:
To solve the question, we write out the chemical equation as follows
NH₄HS (s) ⇄ NH₃ (g) + H₂S (g)
From the above equation, it is observed that only the gaseous products contribute to the partial pressure
Kp =PNH₃·PH₂S where at Kp = 0.070 and PNH₃, PH₂S are the partial pressures of the gases
However since the number of moles of both gases are equal, therefore by Avogadro's law PNH₃ = PH₂S
Then PNH₃ = √(0.07) = PH₂S = 0.2645 atm. ≅ 0.26 atm.
Inertia is the answer to this question
<u>Answer:</u> The partial pressure of hydrogen is 93.9 kPa.
<u>Explanation:</u>
To calculate the partial pressure of hydrogen, we will follow Dalton's Law.
This law states that the total pressure of a mixture of gases is equal to the sum of the individual pressures exerted by the constituent gases.
Mathematically,
According to the question,
We are given:
Putting values in above equation, we get:
Hence, the partial pressure of hydrogen is 93.9 kPa.