Physical change
iron nail have high melting point, thus, when it is heated, it will not melt very easily.
chemical change
iron nail can rust due to the exposure to the air(oxygen). iron in the nail and oxygen in the air will react together to form iron oxide(rust).
furthermore, the reaction is irreversible.
Explanation:
Reaction equation for this reaction is as follows.
It is given that 
= 0.0118.
According to the ICE table,
Initial: 0.86 0.86 0 0
Change: -x -x +x +x
Equilibrium: 0.86 - x 0.86 - x x x
Hence, value of will be calculated as follows.
0.0118 = 
x = 0.084 atm
Thus, we can conclude that 
is 0.084 atm.
Answer:
B) we will convert the 10 g of NaCl into moles.
Explanation:
Molarity is used to describe the concentration of solution. It tells how many moles are dissolve in per litter of solution.
Formula:
Molarity = number of moles of solute / L of solution
we will convert the 10 g of NaCl into moles.
Number of moles of NaCl:
Number of moles = mass/molar mass
Number of moles = 10 g/ 58.44 gmol
Number of moles = 0.17 mol
1 Kg = 1 L
Molarity = 0.17 mol / 2 L
Molarity = 0.085 mol/L
Molarity = 0.085 M
Answer:
its 2p
Explanation:
In a neutral carbon atom, the 1s sublevel has one orbital with two electrons with opposite spins, represented by the arrows pointing in opposite directions. The 2s sublevel also has one orbital with two electrons, also with opposite spins. The 2p sublevel has three orbitals.
(i don"t understand this i just looked it up ._.
This can be done in the following way;
1 determining the heat required to convert 0° C ice to 0°C water
Heat of fusion of water = 334 J/g
Therefore; Heat = 50 g × 334 J/g = 16700 J
2. Determining the heat required to raise the temperature of water from 0° C to 100°C.
Specific heat of water is 4.18 J/g°C
Change in temperature is 100°C
Therefore; Heat = 50 g × 4.18 J/g°C × 100 = 20900 J
3. Determining the heat required to convert 100 ° C water to 100°C vapor
Heat of vaporization of water = 2257 J/g
Heat = Mass of water × heat of vaporization
Heat = 50 g × 2257 = 112850 J
4. Determining the heat required to go from 100° C to 120° vapor
specific heat of vapor = 2.09 J/g°C
Heat = mass × Specific heat of vapor × change in temperature
= 50 g × 2.09 ×(120-100) = 2090 J
Therefore the total heat required is
= 16700 J + 20900 J + 112850 J + 2090 J = 152540 J or 152.54 kJ
