Answer:
8 mol
Explanation:
Step 1: Calculate the mass of PtCl₄ in the sample
10.00 grams of a sample of hydrated PtCl₄ are heated and lose 3.00 g of water. The mass of PtCl₄ is:
mPtCl₄ = 10.00 g - 3.00 g = 7.00 g
Step 2: Calculate the moles corresponding to 7.00 g of PtCl₄ and 3.00 g of H₂O
The molar mass of PtCl₄ is 336.9 g/mol.
7.00 g × 1 mol/336.9 g = 0.0208 mol
The molar mass of H₂O is 18.02 g/mol.
3.00 g × 1 mol/18.02 g = 0.166 mol
The molar ratio of H₂O to PtCl₄ is:
0.166 mol H₂O/0.0208 mol PtCl₄ ≈ 8 mol H₂O/ 1 mol PtCl₄
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Explanation:
CuSO4.5H2O and CaSO4.2H2O
Answer:
Ca(s) + N₂(g) + 3O₂(g) → Ca(NO₃)₂ (s)
Explanation:
The reaction of the formation of Ca(NO₃)₂(s) , is as follows -
Ca + N₂ + O₂ → Ca(NO₃)₂
The above reaction , can be balanced by adding whole numbers ,
Hence , the balanced reaction is as follows -
Ca + N₂ + 3O₂ → Ca(NO₃)₂
The states of the respective molecules is -
the state at which the atoms are most stable or the state at which the atoms are most commonly found .
Hence ,
Calcium is most stable in solid state
Oxygen is most stable in gaseous state
Nitrogen is most stable in gaseous state
hence , the balanced reaction with all the states mentioned is as follows -
Ca(s) + N₂(g) + 3O₂(g) → Ca(NO₃)₂ (s) .
