Answer:
The molar mass of H₂O₂ (the solute) in the aqueous solution of
H₂O₂ is 51 g
Explanation:
Given;
H₂O₂ compound
Concentration of aqueous solution of H₂O₂ = 1.5M
The molecular mass of H₂O₂ = (1 x 2) + (16 x 2) = 34 g/mol
Reacting mass (g) = Concentration x Molar mass
Reacting mass (g) = 1.5 x 34
Reacting mass (g) = 51 g
Therefore, the molar mass of H₂O₂ (the solute) in the aqueous solution of
H₂O₂ is 51 g
Answer: 98.36g/mol
Explanation:Please see attachment for explanation
<u>Answer:</u> The ideal yield of carbon dioxide is 7.506 grams
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
Given mass of carbon monoxide = 5.61 g
Molar mass of carbon monoxide = 28 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of carbon monoxide and water follows:
By Stoichiometry of the reaction:
1 mole of carbon monoxide produces 1 mole of carbon dioxide
So, 0.200 moles of carbon monoxide will produce = of carbon dioxide
Now, calculating the mass of carbon dioxide from equation 1, we get:
Molar mass of carbon dioxide = 44 g/mol
Moles of carbon dioxide = 0.200 moles
Putting values in equation 1, we get:
To calculate the experimental yield of carbon dioxide, we use the equation:
Percentage yield of carbon dioxide = 85.3 %
Theoretical yield of carbon dioxide = 8.8 g
Putting values in above equation, we get:
Hence, the ideal yield of carbon dioxide is 7.506 grams