Answer: decrease the temperature of the reaction
Explanation:
CH3COOH + CH3CH2OH ⇌ CH3COOCH2CH3 + H2O
The formation of an ester is an exothermic reaction. Therefore, a decrease in the temperature of the reaction will favour the production of ester.
The valence electrons in metals. Unlike those in covalently bonded substances
<h2><u>Full Question: </u></h2>
Attached in attachment.
<h2><u>Answer</u>:</h2>
Y is from Group 17. It needs 1 electron to complete its octet. There are total 6 lone pairs in molecule and 1 bond pair. The bond is covalent bond.
<h3><u>Explanation</u>:</h3>
In the picture given, we can see that it contains Lewis Dot structure of two elements X and Y. The X is said as a halogen and also correspondingly has 7 electrons in its outermost shell. The Y isn't mentioned which element it is, but similarly to X it also has 7 electrons in its outermost shell. So it is also a halogen. The group of the halogen is group 17. So Y belongs to group 17.
As the element has 7 electrons in its outermost shell, so it needs 1 electron to fulfill it's octet. It forms a covalent bond with X from where it gets 1 electron via sharing.
So now, there are three unshared electron pair of X and 3 unshared electron pair of Y. So a total of 6 unshared electron pair and 1 bond pair of electron between X and Y.
Answer:
Covalent bonds.
Explanation:
Covalent binds where electrons are shared between the H and O atoms.
1) You will need to use the atomics masses of the elements. So list them:
K: 39 g/mol
C: 12 g/mol
O: 16 g/mol
2) Your base is 100 grams, so you have:
K: 52.1 g
C: 15.8 g
O: 32.1 g
3) Convert grams to moles (dividing each element by its atomic mass)
K: 52.10g / 39 g/mol = 1.336 mol
C: 15.8 g / 12 g/mol = 1.317 mol
O: 32.1 g / 16 g/mol = 2.006 mol
4) Divide all the mol numbers by the least mol number:
K: 1.336 / 1.317 = 1.01
C: 1.317 / 1.317 = 1.00
O: 2.006 / 1.316 = 1.52
5) To have only whole numbers multiply by 2 and round to the nearest whole number
K = 2
C = 2
O = 3
So the empirical formula is K2C2O3
6) Find the molar mass of the empirical formula:
2*39 + 2*12 + 3*16 = 150.
7) Find the number of times that the molecular formula containd the mass of the empirical formula:
150 / 150.22 = 1
Then the molecular formula is the same empirical formula.
Answer: K2C2O3.