Answer:
Mass = 245.72 g
Explanation:
Given data:
Mass of SrCl₂ react = ?
Mass of H₂SO₄ = 300.0 g
Solution:
SrCl₂ + 2H₂SO₄ → 2HCl + Sr(HSO₄)₂
Number of moles of H₂SO₄:
Number of moles = mass/molar mass
Number of moles = 300.0 g/ 98.079 g/mol
Number of moles = 3.1 mol
Now we will compare the moles of SrCl₂ and H₂SO₄.
H₂SO₄ : SrCl₂
2 : 1
3.1 : 1/2×3.1 = 1.55 mol
Mass of SrCl₂:
Mass = number of moles × molar mass
Mass = 1.55 mol × 158.53 g/mol
Mass = 245.72 g
B nitrogen and water vapor<span />
Answer:
True
Explanation:
All the above statements buttress the fact that the larger molecule, the greater the magnitude of London forces between the molecules. Each of the statements above is a confirmation/explanation of this general rule.
Answer:
5.96 g/cm^3
Explanation:
Corner atom = 1/8
Atoms in center = 1
Atoms in face of the cube= 1/2
Molar mass of V = 50.94 g/mol <em>(from period table)</em>
1 mole = 6.02x10^23
<em>In BCC unit cell:</em>
(8 x 1/8)+ 1=2 per 1 unit cell
<em>Mass: </em>2(50.94g)/6.02x10^23 = 1.69x10^-22 g/unit cell
305pm=(305x10^-12m÷10^-2m) x (1mL÷1cm^3)
= 2.837 x 10^-23 mL
<em>1pm=10^-12m</em>
<em>1cm=10^-2m</em>
<em>1mL=1cm^3</em>
<em></em>
density=mass/volume
density of V = 1.69x10^-22g÷2.837x10^-23mL
=5.957g/mL
=5.96g/cm^3
