Answer:
1.63425 × 10^- 18 Joules.
Explanation:
We are able to solve this kind of problem, all thanks to Bohr's Model atom. With the model we can calculate the energy required to move the electron of the hydrogen atom from the 1s to the 2s orbital.
We will be using the formula in the equation (1) below;
Energy, E(n) = - Z^2 × R(H) × [1/n^2]. -------------------------------------------------(1).
Where R(H) is the Rydberg's constant having a value of 2.179 × 10^-18 Joules and Z is the atomic number= 1 for hydrogen.
Since the Electrons moved in the hydrogen atom from the 1s to the 2s orbital,then we have;
∆E= - R(H) × [1/nf^2 - 1/ni^2 ].
Where nf = 2 = final level= higher orbital, ni= initial level= lower orbital.
Therefore, ∆E= - 2.179 × 10^-18 Joules× [ 1/2^2 - 1/1^2].
= -2.179 × 10^-18 Joules × (0.25 - 1).
= - 2.179 × 10^-18 × (- 0.75).
= 1.63425 × 10^- 18 Joules.
Electrostatics is <span> a branch of physics that deals with the phenomena and properties of stationary or slow-moving electric charges. :) Hope this helps </span>
Answer:
B
Explanation: im not rlly sure you can go with what i said or you dont
Answer: 
.
Explanation:
Temperature of the gas is defined as the degree of hotness or coldness of a body. It is expressed in units like 
and 
These units of temperature are inter convertible.
We are given:
Temperature of the gas = 
(1mK=0.001 K)
Converting this unit of temperature into by using conversion factor:
Thus 
Thus the temperature is .
Answer: 
Explanation:
Heat of combustion is the amount of heat released when 1 mole of the compound is completely burnt in the presence of oxygen.
To calculate the moles, we use the equation:
Thus 
of sucrose releases = 916.6 J of heat
1 mole of sucrose releases =
of heat
Thus ∆H value for the combustion reaction is
