Given parameters:
Heat of fusion of water = 334j/g
Mass of ice = 45g
Temperature of ice = 0.0°c
Unknown:
Amount of heat needed to melt = ?
Solution:
This is simply a phase change and a latent heat is required in this process.
To solve this problem; use the mathematical expression below;
H = mL
where m is the mass
L is the heat of fusion of water;
H = 45 x 334 = 15030J
<span>Mass of the solution = 0.17m
Kb for C6H5NH2 = 3.8 x 10^-10
We know Ka for C6H5NH2 = 1.78x10^-11
We have Kw = Ka x Kb => Ka = Kw / Kb
=> (C2H5NH2)(H3O^+)/(C2H5NH3^+) => 1.78x10^-11 = K^2 / 0.17
K^2 = 3 x 10^-12 => K = 1.73 x 10^-6.
pH = -log(Kw(H3O^+)) = -log(1.73 x 10^-6) = 5.76</span>
If i’m not mistaken it must be able to to design an experiment to test a hypothesis
Answer: mass and volume
Explanation:
Divide the mass by the volume in order to get an object's Density.
Answer: The final volume will be 2.89 L.
Explanation:
Given: 
, 
, 
= 101.3 kPa
Convert kPa to atm as follows.
= 1520 torr
Convert torr into atm as follows.
Formula used to calculate final temperature is as follows.
Substitute the values into above formula as follows.
Thus, we can conclude that the final volume will be 2.89 L.
