If you are asking for the word for this definition it is a <span>attraction by the two nucluei</span>
The experimental control is the standard used as a comparison for the experimental groups.
For example, you may be trying to find out how different types of disinfectants affect bacterial growth. The control group would receive <em>no</em> disinfectant whereas the experimental groups would be the ones on which the disinfectants were tested.
Hope this makes sense!
MH₂ = 2×mH = 2×1g = 2 g/mol
<span>The "p" in pH and pOH stands for "negative logarithm of" and is used to make it easier to work with extremely large or small values. pH and pOH are only meaningful when applied to aqueous (water-based) solutions. </span>
Answer:
Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is 45.249 kiloJoules.
Explanation:
Mass of the tin ,m= 425 g
Heat capacity of the tin ,c= 0.227 J/g K
Initial temperature of the tin ,
= 25.0 °C = 298.15 K
Final temperature of the tin,
= 231.9 °C = 505.05 K
Let the heat required to change the temperature of tin from 298.15 K to 505.05 K be Q.
![Q=mc\times (T_2-T_1)](https://tex.z-dn.net/?f=Q%3Dmc%5Ctimes%20%28T_2-T_1%29)
![=425 g\times 0.227 J/g K\times (505.05K - 298.15 K)=19,960.68 J=19.961 kJ](https://tex.z-dn.net/?f=%3D425%20g%5Ctimes%200.227%20J%2Fg%20K%5Ctimes%20%28505.05K%20-%20298.15%20K%29%3D19%2C960.68%20J%3D19.961%20kJ)
Heat required to melt tin at 505.05 K be Q'
The heat of fusion of tin metal =![\Delta H_{fus}=59.2 J/g](https://tex.z-dn.net/?f=%5CDelta%20H_%7Bfus%7D%3D59.2%20J%2Fg)
![Q'= m\times \Delta H_{fus}=425 g\times 59.2 J/g=25,287.5 J=25.288 kJ](https://tex.z-dn.net/?f=Q%27%3D%20m%5Ctimes%20%5CDelta%20H_%7Bfus%7D%3D425%20g%5Ctimes%2059.2%20J%2Fg%3D25%2C287.5%20J%3D25.288%20kJ)
Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is:
= Q+Q' = 19.961 kJ + 25.288 kJ = 45.249 kJ