Answer:
Put the light bulb that was removed back into the circuit and observe whether the other lights come on.
Explanation:
If all three bulbs initially glowed and she supposes that after removing the first bulb, the others stopped glowing because they burned out, then she must replace the original bulb and see if the other two bulbs will glow.
If all three bulbs don't glow after replacing the first one, then all the bulbs may have probably burned out.
the solute is the one that dissolves meaning its particles are separating into the solvent, and the solvent is the one that dissolves the other substance.
Potassium Iodide have a lot of strong bonds which requires a very high temperature (high energy) to break them and change into a different state of matter.
Answer: The empirical formula is H2SO4 only.
Explanation: Because it is the simplest ratio of atoms of elements in a compound.
Answer:
B. Diethyl ether, dichloromethane, ethyl acetate, ethanol
Explanation:
The polarity of solvents can be determined by their polarity indexes. Polarity index is defined as the measure of the ability of the solvent to interact with various polar test solutes.
Diethyl ether is the least polar with a polarity index of 2.8
Dichloromethane with a polarity index of 3.1
Ethyl acetate with a polarity index of 4.3
Ethanol is the most polar with a polarity index of 5.2
The differences in polarities of these solvents is due to their structure. Polar solvents have large dipole moments because they contain bonds between atoms with very different electronegativities, such as oxygen and hydrogen.
Because of the two non-polar methyl groups in diethyl ether, it is not as polar as dichloromethane which has two electronegative chlorine atoms attached to a carbon atom. Similarly too, because diethyl ether has two strongly electronegative oxygen atoms sharing a bond with carbon, it has a larger dipole moment than dichloromethane. Ethanol has an oxygen hydrogen bond which has the largest dipole moment, thus, it is the most polar of the given solvents.
