The enthalpy of combustion of 1 mole of benzene is 3169 kJ/mol .
The first step in answering this question is to obtain the balanced thermochemical equation of the reaction. The thermochemical equation shows the amount of heat lost or gained.
The thermochemical equation for the combustion of benzene is;
2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔrH° = -3169 kJ/mol
We can see that 1 mole of benzene releases about 3169 kJ/mol of heat.
Learn more: brainly.com/question/13164491
:CH=CH2, also expressed as H-C=C:
<span>___________________________|__| </span>
<span>___________________________H H </span>
<span>(Sorry about the underscores; the spacing doesn't work if I don't include them) </span>
<span>This compound is a derivative of ethene, which is CH2=CH2. In place of the fourth H atom, CH3 has a lone pair (as shown in the above formula). Or, it can be bonded to another compound as well in that empty spot.</span>
B it is an aldose to ketose isomerization
Answer:
Explanation:
Atomic radius is the measurement from the nucleus to the outer edge of the electron cloud.
As you go down a group (vertically) the atomic radius increases because more electron shells are added. As you go across a period horizontally, the atomic radius decreases.
If we look at the halogens group (17), we see they follow this order from top to bottom:
F - Fluorine
Cl - Chlorine
Br - Bromine
I - Iodine
Since it increases down the group, iodine must have the largest atomic radius.
Cover your mouth and nose with a face mask or other material (such as a scarf or handkerchief) until the fallout cloud has passed.
