Answer:
the reaction is spontaneous at T > 2900 K
Explanation:
∴ ΔH = +120 KJ
∴ ΔS = (-42 J/K)*(KJ/1000 J) = -0.042 KJ/K
∴ ΔG < 0 ⇒ the reaction is spontaneous
⇒ at T = 2900 K:
⇒ ΔG = 120 - (2900)(-0.042) = 120 - 121.8 = - 1.8 KJ < 0
Answer:
O2 and O3 are allotropes of Oxygen, therefore they have (4) different chemical and physical properties.
Explanation:
Answer:
Mass of Cl₂ produced 12.78 g
Explanation:
Given data:
Mass of MnO₂ = 16 g
Mass of HCl = 30.0 g
Mass of Cl₂ produced = ?
Solution:
Chemical equation:
MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O
Number of moles of MnO₂:
Number of moles = mass / molar mass
Number of moles = 16 g/ 87 g/mol
Number of moles = 0.18 mol
Number of moles of HCl:
Number of moles = mass / molar mass
Number of moles = 30 g/ 36.46 g/mol
Number of moles = 0.82 mol
Now we will compare the moles of Cl₂ with MnO₂ and HCl.
MnO₂ : Cl₂
1 : 1
0.18 : 0.18
HCl : Cl₂
4 : 1
0.82 : 1/4×0.82 = 0.205 mol
The number of moles of Cl₂ formed by HCl are less it will limiting reactant.
Mass of Cl₂ formed:
Mass = number of moles × molar mass
Mass = 0.18 mol × 71 g/mol
Mass = 12.78 g
First, we have to get moles of Mg2+ = molarity * volume
= 1 x 10^-2 * 0.15 L
= 0.0015 mol
initial [Mg2+] = 0.0015 / 0.4 L(total volume)
= 0.00375 M
then, moles of F- = molarity * volume
= 1 x 10^-1 * 0.25
= 0.025 Mol
initial [F-] = 0.025 / 0.4 = 0.0625 M
by using ICE table:
MgF2(s) → Mg2 + 2F-
initial 0.00375 0.0625
change + X +2 X
Equ 0.00375+X 0.0625+2X
when Ksp = [Mg2+][F-]^2
by substitution:
6.4 x 10^-9 = (0.00375+X)( 0.0625 +2X)^2 by solving for X
∴X= 0.00024 M
∴[Mg2+] = 0.00375 + X
= 0.00375 + 0.00024
= 0.004 M
and [F-] = 0.0625 + 2X
= 0.0625 + 2* 0.00024
= 0.06 M
<h2>Answer:</h2>
4. becomes softer as temperature rises
<h2>Explanation:</h2>
An amorphous solid is any noncrystalline solid in which the atoms and molecules are not organized in a definite lattice pattern. Such solids include glass, plastic, and gel. Solids and liquids are both forms of condensed matter; both are composed of atoms in close proximity to each other.
