The value of X is 2
The total amount of sample taken is 2.00 g
The amount of sample left in the oven after drying is 1.565g
The amount of sample lost (mass of water driven out) = Total sample-Anhydrous salt left in the oven
= 2.00 - 1.565
= 0.435 grams
The moles of anhydrous salt present in the hydrate = 1.565g/129.83g/mol = 0.01205
The moles of water present in the hydrate = 0.4350g/18.01g/mol = 0.02415
Therefore the ratio of these two are in 1:2 ratio
The complete chemical reaction is CoCl2.2H20
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Answer:
![Molarity_{Cl^-}=1.434\ M](https://tex.z-dn.net/?f=Molarity_%7BCl%5E-%7D%3D1.434%5C%20M)
Explanation:
Moles of NaCl :
Given, Mass of NaCl = 72.24 g
Molar mass of NaCl = 58.44 g/mol
The formula for the calculation of moles is shown below:
Thus,
![Moles\ of\ NaCl= 1.2361\ mol](https://tex.z-dn.net/?f=Moles%5C%20of%5C%20NaCl%3D%201.2361%5C%20mol)
NaCl is a strong salt. So, moles of chloride ion = 1.2361 moles
Volume = 0.862 L
![Molarity_{Cl^-}=1.434\ M](https://tex.z-dn.net/?f=Molarity_%7BCl%5E-%7D%3D1.434%5C%20M)
Answer:
0.174kg of Ore are required
Explanation:
The ore of 37.3% in nickel by mass means that <em>in 100g of ore there are 37.3g of nickel. </em>As we need to obtain 65g of nickel we can convert this mass to mass of ore using the conversion factor (100g Ore / 37.3g Nickel) as follows:
65g of nickel * (100g Ore / 37.3g Nickel) = 174g of Ore are needed to have 65.0g of nickel. In kilograms:
174g Ore * (1kg / 1000g) =
<h3>0.174kg of Ore are required</h3>
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