All categories

3 years ago

Compare the reactivity of alcohols with the length of the R-group.

2 answers:

6 0

As you increase the chain of a alcohol, the reactivity decreases. This is due to an increase in disorder and decrease in intermolecular attraction between molecules.

soldier1979 [14.2K]3 years ago

3 0

As you increase the chain of alcohol, the reactivity decreases.

You might be interested in

The density of ethanol, a colorless liquid that is commonly known as grain alcohol, is 0.798 g/ml. calculate the mass of 16.9 ml

sesenic [268]

Hey there!:

Density = 0.798 g/mL

Volume = 16.9 mL

Therefore:

Mass = density * volume

Mass = 0.798 * 16.9

Mass = 13.4862 g

4 0

3 years ago

Given KNO3 + CuSO4 is a double replacement reaction, predict the products and then determine whether you would expect to see a p

slava [35]

Answer:

Products will be K2SO4 and Cu(NO3)2. A precipitate will not form.

Explanation:

Double replacement reactions are the switching of cations between two compounds. So in this case, the K+ and Cu 2+ cations will switch places.

KNO3 + CuSO4 -> K2SO4 + Cu(NO3)2

According to solubility rules, any substances containing NO3 or a Group 1 ion (K+ in this case) will be definitely soluble. There are a few exceptions to the Group 1 rule but it does not apply here. Potassium sulfate (K2SO4) contains a Group 1 ion so it will be soluble and not be a precipitate. And copper nitrate (Cu(NO3)2) contains nitrate so it will also be soluble and not be a precipitate.

4 0

3 years ago

The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and oxygen. A 2.001 g sample of B

Alborosie

Answer: The empirical formula for the given compound is $C_{15}H_{24}O_1$

Explanation:

The chemical equation for the combustion of compound having carbon, hydrogen, iron and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=5.995g$

Mass of $H_2O=1.963g$

Mass of sample = 2.001 g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 5.995 g of carbon dioxide, $\frac{12}{44}\times 5.995=1.635g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 1.963 g of water, $\frac{2}{18}\times 1.963=0.218g$ of hydrogen will be contained.

Mass of oxygen in the compound = (2.001) - (1.635 + 0.218) = 0.148 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.635g}{12g/mole}=0.136moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.218g}{1g/mole}=0.218moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.148g}{16g/mole}=0.0092moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0092 moles.

For Carbon = $\frac{0.136}{0.0092}=14.78\approx 15$

For Hydrogen = $\frac{0.218}{0.0092}=23.69\approx 24$

For Oxygen = $\frac{0.0092}{0.0092}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 15 : 24 : 1

Hence, the empirical formula for the given compound is $C_{15}H_{24}O_1$

3 0

4 years ago

Cohesion is the tendency for the same type of molecules to stick together. TRUE or FALSE

Sergio039 [100]

True

cohesion is the tendency for the same type of molecules to stick together!

5 0

3 years ago

A particular flask has a mass of 17.4916 g when empty. When filled with ordinary water at 20.0°c (density = 0.9982 g/ml), the ma

LUCKY_DIMON [66]

The mass of the empty flask is 17.4916 g. Now after feeling the ordinary water the mass of the flask is 43.9616 g. Thus the change of weight due to addition of ordinary water is (43.9616 - 17.4916) = 26.47 g.

Now as the density of the ordinary water at 20°C is 0.9982 g/ml, so 26.47 g is equivalent to $\frac{26.47}{0.9982}=26.5177$ mL of water. Thus the capacity of the flask is 26.5177 mL.

Now the density of heavy water is 1.1053 g/mL at 20°C. Thus 26.5177 mL of heavy water is equivalent to (1.1053×26.5177) = 29.310 g.

Thus the total weight of the flask filled with heavy water will be (17.4916 + 29.310) = 46.8016 g at 20°C.

4 0

3 years ago

Read 2 more answers