moles are in 1.30 mL of acetic anhydride given that the density of acetic anhydride is 1.08 g/mL and the molecular weight is 102 g/mol?
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To find the number of moles in 1.30 mL of acetic anhydride, we'll follow these steps:
Step 1: Calculate the mass of acetic anhydride in 1.30 mL.
Mass = density x volume
Mass = 1.08 g/mL x 1.30 mL
Step 2: Calculate the number of moles using the molecular weight of acetic anhydride.
Number of moles = mass / molecular weight
Number of moles = (1.08 g/mL x 1.30 mL) / 102 g/mol
Now, let's calculate:
Mass = 1.08 g/mL x 1.30 mL
Mass = 1.404 g
Number of moles = (1.404 g) / 102 g/mol
Therefore, there are approximately 0.01376 moles in 1.30 mL of acetic anhydride.
To determine the number of moles in 1.30 mL of acetic anhydride, we need to follow these steps:
1. Calculate the mass of the given volume of acetic anhydride using the density:
Mass = Volume x Density
= 1.30 mL x 1.08 g/mL
= 1.404 g
2. Next, we can convert the mass of acetic anhydride into moles using its molecular weight:
Moles = Mass / Molecular Weight
= 1.404 g / 102 g/mol
≈ 0.0138 mol
Therefore, there are approximately 0.0138 moles of acetic anhydride in 1.30 mL of the solution.