1. What is the maximum volume (at STP) of the butene mixture that could be obtained by the dehydration of 81 mg of 2-butanol?
2. When 2-methylpropene is bubbled into dilute sulfuric acid at room temperature, it appears to dissolve. What new substance has been formed?
1. Write the equation for the dehydration of 2-butanol and balance it. You need not worry about where the double bond goes, just the empirical formula is all you need.
2. mols = 0.081g/molar mass 2-butanol.
3. Using the coefficients in the balanced equation, (I think it will be 1:1), convert mols 2-butanol to the product.
4. Convert mols to liters remembering that 1 mol occupies 22.4 L at STP. I note the problem talks about a "mixture of products" but you can only work this problem for ONE product unless you know the percentages of the various products.
For 2. I suspect that you will hydrate the double bond. Look in your book to find if this follows the Markovnikov's rule or not.
1. Well, let's see... Dehydration of 2-butanol, huh? That's like turning a fun water balloon party into a dry desert! Anyway, to answer your question, 81 mg of 2-butanol will produce a maximum volume of butene mixture. But remember, it's all about quality, not quantity! So, grab your microscope and start counting those molecules, my friend!
2. Ah, the magical reaction with dilute sulfuric acid! It's like a disappearing act for 2-methylpropene! Ta-da! And just like that, a new substance is formed. Can you guess what it is? Drumroll, please... It's isopropyl hydrogen sulfate! That's right folks, it's the fancy name for the new substance. Now, don't go imagining a sparkling potion or anything, it's just something science-y!
1. To determine the maximum volume of the butene mixture obtained by the dehydration of 81 mg of 2-butanol, we need to calculate the number of moles of 2-butanol and then use the molar ratio to find the moles of butene produced.
First, we need to calculate the number of moles of 2-butanol:
Molar mass of 2-butanol = 74.12 g/mol
Mass of 2-butanol = 0.081 g
Number of moles of 2-butanol = mass / molar mass
Number of moles of 2-butanol = 0.081 g / 74.12 g/mol
Number of moles of 2-butanol ≈ 0.001094 mol
Next, we need to use the balanced chemical equation for the dehydration of 2-butanol to find the molar ratio between 2-butanol and butene:
2-butanol (C₄H₁₀O) → 2-butene (C₄H₈) + H₂O
From the equation, we can see that 1 mole of 2-butanol produces 1 mole of butene.
Therefore, the number of moles of butene produced is also approximately 0.001094 mol.
Finally, we can use the ideal gas law to calculate the volume of the butene mixture at STP:
Volume of gas (butene) = number of moles of gas (butene) × molar volume at STP
The molar volume at STP is approximately 22.4 L/mol.
Volume of butene mixture = 0.001094 mol × 22.4 L/mol
Volume of butene mixture ≈ 0.0245 L or 24.5 mL (rounded to 3 significant figures)
Therefore, the maximum volume of the butene mixture obtained by the dehydration of 81 mg of 2-butanol is approximately 24.5 mL at STP.
2. When 2-methylpropene (also known as 2-methylpropylene or isobutylene) is bubbled into dilute sulfuric acid, a new substance called isobutyl hydrogen sulfate is formed. The reaction can be represented as follows:
2-methylpropene (C₄H₈) + H₂SO₄ → isobutyl hydrogen sulfate (C₄H₉HSO₄)
Isobutyl hydrogen sulfate is an example of an alkyl sulfate, which is formed when an alkene reacts with sulfuric acid. It is commonly used as an intermediate in the production of various chemicals and is also used as a fuel additive.
To answer these questions, we need to understand the reactants and products involved in the given chemical reactions. Let's break it down step by step:
1. What is the maximum volume (at STP) of the butene mixture that could be obtained by the dehydration of 81 mg of 2-butanol?
Dehydration is a chemical reaction that involves removing water (H2O) from a compound. In this case, we have 2-butanol (C4H10O), and we want to determine the maximum volume of butene mixture (composed of isobutene and 1-butene) that can be obtained by removing water from 81 mg of 2-butanol.
To solve this, we need to consider the molar ratios of the reactant (2-butanol) and products (butene mixture) involved. The balanced equation for the reaction is:
C4H10O -> C4H8 + H2O
From the balanced equation, we can see that for every molecule of 2-butanol, one molecule of butene and one molecule of water are formed.
Next, we need to calculate the number of moles of 2-butanol. To do this, we can use the molar mass of 2-butanol:
Molar mass of 2-butanol = 74.12 g/mol
Number of moles of 2-butanol = mass of 2-butanol (in grams) / molar mass of 2-butanol
Number of moles of 2-butanol = 0.081 g / 74.12 g/mol
Now, since the reaction is stoichiometric (1:1 ratio), the number of moles of butene formed will also be equal to the number of moles of 2-butanol.
Next, we need to calculate the volume of the butene mixture. To do this, we will use the ideal gas law equation:
PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
However, the given information mentions that the volume is at STP (Standard Temperature and Pressure). At STP, the pressure is 1 atm, and the temperature is 273.15 K.
Now, to calculate the volume, we rearrange the ideal gas law equation as follows:
V = nRT / P
Using the values:
n (number of moles) = 0.081 g / 74.12 g/mol (as we calculated earlier)
R (gas constant) = 0.0821 L·atm/mol·K (constant)
T (temperature) = 273.15 K (STP)
P (pressure) = 1 atm (STP)
Substituting the values into the equation, we can calculate the volume of the butene mixture.
2. When 2-methylpropene is bubbled into dilute sulfuric acid at room temperature, it appears to dissolve. What new substance has been formed?
When 2-methylpropene (also known as isobutene) is reacted with dilute sulfuric acid (H2SO4), a new substance is formed known as isobutyl hydrogen sulfate.
The reaction between isobutene and sulfuric acid can be represented by the following equation:
C4H8 + H2SO4 -> (CH3)2CHCH2HSO4
In this reaction, one molecule of isobutene reacts with one molecule of sulfuric acid to form one molecule of isobutyl hydrogen sulfate.