Answer:
Option A.
Lower air pressure results in a lower boiling point
Explanation:
This is because in an open system, the lower the pressure the lesser the energy that will be required for boiling point. The is little or no collision of air molecules with the surface of the liquid
But if there is increase in pressure, more energy will be required to get to boiling point because there will be strong collision between air molecules and surface of the liquid.
Answer:
A balanced chemical equation follows law of conservation of mass. This law states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form. This means that total mass on the reactant side is equal to the total mass on the product side.
Answer:
45.4 L
Explanation:
Using Ideal gas equation for same mole of gas as
Given ,
V₁ = 27.9 L
V₂ = ?
P₁ = 732 mmHg
P₂ = 385 mmHg
T₁ = 30.1 ºC
T₂ = -13.6 ºC
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (30.1 + 273.15) K = 303.25 K
T₂ = (-13.6 + 273.15) K = 259.55 K
Using above equation as:
Solving for V₂ , we get:
<u>V₂ = 45.4 L</u>
