An "inch of mercury" (written as inHg) is used to measure atmospheric pressure.
2MnO4-(aq) + 16H+ + 10Cl-(aq) ⇔ 2Mn2+(aq) + 8H2O + 5Cl2 (g)
<h3>Further explanation</h3>
Given
Reaction(unbalanced)
Mno4- (aq) + Cl- (aq) → Mn2+ + Cl2 (g)
Required
Half reaction
Solution
1. Add coefficient(equalizing atoms in reaction)
2. Adding H₂O on the O-deficient side.
3. Adding H⁺ on the H-deficient side.
4. Adding e⁻
5. Equalizing the number of electrons and sum the all the half-reaction
1.MnO₄⁻(aq) = Mn²⁺(aq) reduction
2.MnO4(aq) = Mn2+(aq) + 4H2O
3. MnO4-(aq) + 8H+ = Mn2+(aq) + 4H2O
4. MnO4-(aq) + 8H+ + 5e- = Mn2+(aq) + 4H2O
Cl⁻(aq) = Cl₂(g) oxidation
1. 2Cl-(aq) = Cl2 (g)
2-3 none
4. 2Cl-(aq) = Cl2 (g) + 2e-
5.
MnO4-(aq) + 8H+ + 5e- = Mn2+(aq) + 4H2O x2
2Cl-(aq) = Cl2 (g) + 2e- x5
2MnO4-(aq) + 16H+ + 10e- = 2Mn2+(aq) + 8H2O
10Cl-(aq) = 5Cl2 (g) + 10e-
<em>2MnO4-(aq) + 16H+ + 10Cl-(aq) ⇔ 2Mn2+(aq) + 8H2O + 5Cl2 (g)</em>
Do you need to know from solid to liquid,liquid to gas or gas to liquid?
Answer:
168.4 mL
Explanation:
Data Given
initial volume V1 of gas in balloon = 100 mL
initial pressure P1 of gas in balloon = 3.2 atm
final pressure P2 of gas in balloon = 1.9 atm
final volume V2 of gas in balloon = ?
Solution:
This problem will be solved by using Boyle's law equation at constant Temperature.
The formula used
P1V1 = P2V2
As we have to find out Volume, so rearrange the above equation
V2 = P1V1 / P2
Put value from the data given
V2 = 100 mL x 3.2 atm / 1.9 atm
V2 = 168.4 mL
So the final Volume of gas in baloon = 168.4 mL
The observation that indicates that the kinetic-molecular theory has limited use for describing a certain gas is that gas particles are obeying Newton's laws of motion. The correct answer is B.
