Answer:
why cant you just say the grasshopper eats the marsh grass the shrew eats the grasshopper and the hawk eats the shrew.
Explanation:
this makes sense to me but im not sure.
On the lab the text is kind of too far zoomed out so u can’t really read it it’s like blurry
Answer:
% (COOK)2H2O = 37.826 %
Explanation:
mix: (COOK)2H2O + Ca(OH)2 → CaC2O4 + H2O
∴ mass mix = 4.00 g
∴ mass (CaC2O4)H2O = 1.20 g
∴ Mw (COOK)2H2O = 184.24 g/mol
∴ Mw (CaC2O4)H2O = 146.12 g/mol
∴ r = mol (COOK)2H2O / mol (CaC2O4)H2O = 1
- % (COOK)2H2O = (mass (COOK)2H2O / mass Mix) × 100
⇒ mass (COOK)2H2O = (1.20 g (CaC2O4)H2O)×(mol (CaC2O4)H2O / 146.12 g (CaC2O4)H2O)×(mol (COOK)2H2O/mol (CaC2O4)H2O)×(184.24 g (COOK)2H2O/mol (COOK)2H2O)
⇒ mass (COOK)2H2O = 1.513 g
⇒ % (COOK)2H2O = ( 1.513 g / 4 g )×100
⇒ % (COOK)2H2O = 37.826 %
Answer:
MgSO4. 7H2O
There are seven water molecules attached to the hydrated salt.
Explanation:
From the equation;
Number of moles of hydrated salt = number of moles of anhydrous salt, we obtain:
Mass of hydrated salt/ molar mass of hydrated salt = mass of anhydrous salt/ molar mass of anhydrous salt
From the question;
Mass of hydrated salt = 1.000g
Molar mass of hydrated salt = 120.366 +18x gmol-1
Mass of anhydrous salt= 0.488g
Molar mass of anhydrous salt= 120.366 gmol-1
Substituting into the equation above;
1.000/120.366 +18x = 0.488/120.366
1.000/120.366 +18x = 0.004
1.000= 0.004 (120.366 +18x)
1.000= 0.48 + 0.072x
1.000 - 0.48 = 0.072x
0.52= 0.072x
x= 0.52/0.072
x=7
Therefore the hydrated salt is MgSO4. 7H2O
