It requires 334 kJ of heat to melt 1 kg of ice. The largest known iceberg had a volume of about 3.1 x 10^13 m³. How much heat wa
s required
to melt the iceberg if 1 m³ of ice has a mass of 917 kg?
to melt the iceberg if 1 m³ of ice has a mass of 917 kg?
1 answer:
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The given compound is
Each formula unit of has 2 mol Potassium (K) atoms, 2 mol Chromium (Cr) atoms and 7 mol Oxygen (O) atoms.
Atomic weight of potassium is 39.0983 amu
Atomic weight of Chromium is 51.9961 amu
Atomic weight of Oxygen is 15.9994 amu.
Therefore the formula weight of
= 294.1846 amu
Answer:
1.457*10^-8 grams
Explanation:
First we want to find the molar concentration of MgF2. We can do this by dividing 0.016 (the solubility in grams of MgCl2 in a litre of water) by its molar mass (approx. 62.3 grams). Thus, the molar solubility of MgF2 is 2.57*10^-4 M.
Next, we must calculate the Ksp of MgF2. The equilibrium expression is:
MgF2⇄Mg+2F
Thus
This means that, in equilibrium, there are 2.57*10^-4 M of and 5.136*10^-4 M of
Plugging in the above information, our Ksp for MgF2 is approximately 6.78*10^-11
Next we will need to use the RICE table. Since there is already 0.29M of NaF dissolved, there is initially 0.29M of .
R: MgF2 ⇄ +2
I: N/A 0 0.29M
C: N/A +x +x
--------------------------------------------
E: N/A x 0.29+x
To make calculations easier, we will assume that 0.29+x≈0.29
This means that Ksp=0.29x=6.78*10^-11
Therefore, x≈2.338*10^-10M
Multiply that by 62.3 and we get around 1.457*10^-8 grams.