I'm certain it's "D"
...because it can't be "A" or "B" because solubility IS a property but to actually determine whether these two substances are the same or different we would need at least two-three properties (like boiling point or specific heat).
and it can't be "C" because the melting point is just simply irrelevant when comparing the solubility of two substances.
Molarity = number of moles of solute/liters of solution
number of moles of solute = molarity x liters of solution
Part (a): <span>30.00 ml of 0.100m Cacl2
number of moles of CaCl2 = 0.1 x 0.03 = 3x10^-3 moles
1 mole of CaCl2 contains 2 moles of chlorine, therefore 3x10^-3 moles of CaCl2 contains 6x10^-3 moles of chlorine
Part (b): </span><span>10.0 ml of 0.500m bacl2
number of moles of BaCl2 = 0.5 x 0.01 = 5x10^-3 moles
1 mole of BaCl2 contains 2 moles of chlorine, therefore 5x10^-3 moles of BaCl2 contains 10x10^-3 moles of chlorine
Part (c): </span><span>4.00 ml of 1.000m nacl
number of moles of NaCl = 1 x 0.004 = 0.004 moles
1 mole of NaCl contains 1 mole of chlorine, therefore 4x10^-3 moles of NaCl contains 4x10^-3 moles of chlorine
Part (d): </span><span>7.50 ml of 0.500m fecl3
number of moles of FeCl3 = 0.5 x 0.0075 = 3.75x10^-3 moles
1 mole of FeCl3 contains 3 moles of chlorine, therefore 3.75x10^-3 moles of FeCl3 contains 0.01125 moles of chlorine
Based on the above calculations, the correct answer is (d)</span>
Answer:
1.22 mL
Explanation:
Let's consider the following balanced reaction.
2 AgNO₃ + BaCl₂ ⇄ Ba(NO₃)₂ + 2 AgCl
The molar mass of silver chloride is 143.32 g/mol. The moles corresponding to 0.525 g are:
0.525 g × (1 mol/143.32 g) = 3.66 × 10⁻³ mol
The molar ratio of AgCl to BaCl₂ is 2:1. The moles of BaCl₂ are 1/2 × 3.66 × 10⁻³ mol = 1.83 × 10⁻³ mol.
The volume of 1.50 M barium chloride containing 1.83 × 10⁻³ moles is:
1.83 × 10⁻³ mol × (1 L/1.50 mol) = 1.22 × 10⁻³ L = 1.22 mL
This name is phosphine flammable , toxic gas colourless
...it's formula is PH3
Answer:
- <u>259,000 g of chalk.</u>
Explanation:
<u>1) Data:</u>
a) 2000 boxes
b) 175 g / box
c) % yield = 74%
<u>2) Formula: </u>
- % yield = (theoretical yield / actual yield) × 100
<u>3) Solution:</u>
a) Calcualte the actual yield:
- mass of product = 2000 box × 175 g/ box = 350,000 g
b) Solve for the theoretical yield from the % yield formula:
- % yield = (theoretical yield / actual yield) × 100
⇒ theoretical yield = % yield × actual yield / 100
theoretical yield = 74% × 350,000g / 100 = 259,000 g
