Answer:
23.14 L
Explanation:
Please see the step-by-step solution in the picture attached below.
Hope this answer can help you. Have a nice day!
Answer : The mass of potassium phosphate needed will be 3.98 grams.
Explanation : Given,
Molarity of potassium phosphate = 0.75 M = 0.75 mole/L
Molar mass of potassium phosphate = 212.27 g/mole
Volume of solution = 25.0 mL = 0.025 L (conversion used : 1 L = 1000 mL)
Molarity : It is defined as the number of moles of solute present in one liter of solution.
In this problem solute is, potassium phosphate.
Formula used :
![\text{Molarity}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{volume of solution in liter}}](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20solute%7D%7D%7B%5Ctext%7BMolar%20mass%20of%20solute%7D%5Ctimes%20%5Ctext%7Bvolume%20of%20solution%20in%20liter%7D%7D)
Now put all the given values in this formula, we get:
![0.75mol/L=\frac{\text{Mass of solute}}{212.27g/mole\times 0.025L}](https://tex.z-dn.net/?f=0.75mol%2FL%3D%5Cfrac%7B%5Ctext%7BMass%20of%20solute%7D%7D%7B212.27g%2Fmole%5Ctimes%200.025L%7D)
![\text{Mass of solute}=3.98g](https://tex.z-dn.net/?f=%5Ctext%7BMass%20of%20solute%7D%3D3.98g)
Therefore, the mass of potassium phosphate needed will be 3.98 grams.
Answer : The specific heat of fools gold is
.
Solution : Given,
Molar specific heat of fools gold = ![25.418J/mol^oC](https://tex.z-dn.net/?f=25.418J%2Fmol%5EoC)
Formula weight of fools gold = 119.98 g/mole
Formula used :
Molar specific heat substance = Specific heat of substance × Formula weight of substance
Now we have to calculate the specific heat of fools gold.
![\text{ Specific heat of fools gold}=\frac{\text{ Molar specific heat of fools gold}}{\text{ Formula weight of fools gold}}](https://tex.z-dn.net/?f=%5Ctext%7B%20Specific%20heat%20of%20fools%20gold%7D%3D%5Cfrac%7B%5Ctext%7B%20Molar%20specific%20heat%20of%20fools%20gold%7D%7D%7B%5Ctext%7B%20Formula%20weight%20of%20fools%20gold%7D%7D)
Now put all the given values in this formula, we get
![\text{ Specific heat of fools gold}=\frac{25.418J/mol^oC}{119.98g/mole}=0.21185J/g^oC](https://tex.z-dn.net/?f=%5Ctext%7B%20Specific%20heat%20of%20fools%20gold%7D%3D%5Cfrac%7B25.418J%2Fmol%5EoC%7D%7B119.98g%2Fmole%7D%3D0.21185J%2Fg%5EoC)
Therefore, the specific heat of fools gold is
.
In an endothermic reaction products are <u>HIGHER </u>than reactants in potential energy and <u>LESS </u>stable.
Explanation:
Energy is input into the reaction in an endothermic reaction. This means the products are of a higher energy level than the reactants. Therefore the reaction increases Gibb's free energy and reduces entropy. Remember in thermodynamic stability involves an increase in entropy and a decrease in Gibbs free energy. Therefore the products are less stable than the reactants. This is why endothermic reactions do not occur spontaneously like exothermic reactions.
A homogenous mixture is uniform and thus hard to recognize as a mixture. An example is water.