Answer:
23.0733 L
Explanation:
The mass of hydrogen peroxide present in 125 g of 50% of hydrogen peroxide solution:
Mass = 62.5 g
Molar mass of = 34 g/mol
The formula for the calculation of moles is shown below:
Thus, moles are:
Consider the given reaction as:
2 moles of hydrogen peroxide decomposes to give 1 mole of oxygen gas.
Also,
1 mole of hydrogen peroxide decomposes to give 1/2 mole of oxygen gas.
So,
1.8382 moles of hydrogen peroxide decomposes to give
So,
Pressure = 746 / 760 atm = 0.9816 atm
Temperature = 27 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (27 + 273.15) K = 300.15 K
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
0.9816 atm × V = 0.9191 mol × 0.0821 L.atm/K.mol × 300.15 K
<u>⇒V = 23.0733 L</u>
Answer is: the collision theory.
The collision theory states that a certain fraction of the collisions (successful collisions) cause significant chemical change.
The successful collisions must have enough energy (activation energy), on this diagram that energy is represented with arrow up.
Chemical bonds are broken (between blue and red-black molecules) and new bonds are formed (between blue-red and blue-black molecules), as it is represented on diagram.
Answer:
0.369M
Explanation:
☆ Volume has to be in litres
Molarity of solution
= 0.99 ÷2.5
= 0.369 M
Answer:
Potassium
Explanation:
Most reactive metal in the reactivity series