<span>4.3065 g
To begin with, consult the atomic masses for each involved element.
Atomic weight of Calcium = 40.078
Atomic weight of Carbon = 12.0107
Atomic weight of Hydrogen = 1.00794
Atomic weight of Oxygen = 15.999
Atomic weight of Sulfur = 32.065
Next, compute the molar masses of both reactants and the product.
Molar mass H2SO4 = 2 * 1.00794 + 32.065 + 4 * 15.999
= 98.07688 g/mol
Molar mass CaCO3 = 40.078 + 12.0107 + 3 * 15.999
= 100.0857 g/mol
Molar mass CaSO4 = 40.078 + 32.065 + 4 * 15.999
= 136.139 g/mol
The balanced equation for the reaction between H2SO4 and CaCO3 is:
CaCO3 + H2SO4 ==> CaSO4 + H2O + CO2
Thus, 1 mole each of CaCO3 and H2SO4 is necessary to generate 1 mole of CaSO4. Let's check the amount of moles we have for CaCO3 and H2SO4.
CaCO3: 3.1660 g / 100.0857 g/mol = 0.031632891 mol
H2SO4: 3.2900 g / 98.07688 g/mol = 0.033545113 mol
H2SO4 is in slight excess, therefore CaCO3 is the limiting reactant, suggesting we can expect 0.031632891 moles of product. To find the mass, multiply the number of moles by the molar mass calculated previously.
0.031632891 mol * 136.139 g/mol = 4.306470148 g
Given that we have 5 significant figures from our data, we round the final result to 5 figures, yielding 4.3065 g</span>
Answer:
Explanation:
The percent composition indicates the mass percentage of a specific element within the compound.
The chemical formula for chromium(III) nitrate is 
.
The molar mass for chromium(III) nitrate is calculated at 238.011 g/mol.
Each mole of chromium(III) nitrate includes 9 moles of oxygen.
The molar mass of oxygen is 16 g/mol.
Hence, Mass = Molar mass * Moles = 16 * 9 g = 144 g.
Answer:
The designation of 70% (vol/vol) indicates
that it contains 70% (vol/vol), meaning 70 ml of isopropanol is included in 100 ml of rubbing alcohol solution.
If it were 200 ml, then naturally, it would contain 70*2 = 140 ml of isopropanol required.
Answer: Servsafe 9
Explanation:
Take food off the surface
clean the area
rinse the area
sanitize the area
let the area dry naturally
