Answer:
1.3 × 10⁴ mL
Explanation:
A Pb-contaminated water sample contains 0.0012 %Pb by mass, that is, there are 0.0012 g of Pb in 100 g of solution. The mass of the sample that contains 150 mg (0.150 g) of Pb is:
0.150 g Pb × (100 g sample/0.0012 g Pb) = 1.25 × 10⁴ g sample
The density of the sample is 1.0 g/mL. The volume of the sample is:
1.25 × 10⁴ g × (1 mL/1.0 g) = 1.3 × 10⁴ mL
Answer:
ionic bonding or covalent
Explanation:
Determine the mass of each of the following amounts. a. 1.366 mol of
NH3
, b. 0.120 mol of glucose,
C6H12O6
, c. 6.94 mol barium chloride,
BaCl2
, d. 0.005 mol of propane,
C3H8
Formation of a precipitate
From the balanced equation, we can see that 1 mole of CH4
releases 802.3 kJ of heat upon combustion. The mass of 1 mole of CH4 is:
mass CH4 = 16.04 grams
So by ratio and proportion:
mass required = (-268 kJ) / (-802.3 kJ / 16.04 grams)
<span>mass required = 0.334 grams</span>