Answer:
+3·F
Explanation:
The number of objects in the given system = 2 objects
The charge on each object are; q₁ = -Q, q₂ = -Q
The force acting between the objects = +F
The distance between the objects = 2·d
The formula for the force acting between two charged particles is given as follows;
Therefore, we get;
By tripling the charge, q₁, on the first object, we get;
q₂ = 3 × (-Q)
Therefore, the new force between them, F₂ = +3·F
at equilibrium.
<h3>Explanation</h3>
Concentration for each of the species:
There was no Y to start with; its concentration could only have increased. Let the change in be .
Make a table.
Two moles of X will be produced and two moles of Z consumed for every one mole of Y produced. As a result, the <em>change</em> in will be and the <em>change</em> in will be .
.
Add the value in the C row to the I row:
.
What's the equation of for this reaction? Raise the concentration of each species to its coefficient. Products go to the numerator and reactants are on the denominator.
.
. As a result,
.
.
The degree of this polynomial is three. Plot the equation on a graph and look for any zeros. There's only one zero at . All three concentrations end up greater than zero.
Hence the equilibrium concentration of Y: .
Answer:
Rb
Explanation:
Second ionization energy is the energy required for the removal of the second loosely bonded valence electron from an isolated gaseous atom.
The given elements:
Rb , Sr, Y and Zr
These are the elements of the fifth period.
The electronic configuration of Rb -
The electronic configuration of Sr -
The electronic configuration of Y -
The electronic configuration of Zr -
<u>When one electron is removed from Rb, the cation attains the noble gas configuration due to which the removal of second electron from Rb is very very difficult. Thus, Rb has the largest second ionization energy.</u>
The values of the second ionization of these elements are:
Rb = 2633 kJ/mol
Sr = 1064.2 kJ/mol
Y = 1180 kJ/mol
Zr = 1270 kJ/mol
Answer:
moles
Explanation:
We are given:
Vapor pressure of water = 19.8 torr
Total vapor pressure = 752 torr
Vapor pressure of oxygen gas = Total vapor pressure - Vapor pressure of water = (752 - 19.8) torr = 732.2 torr
To calculate the amount of oxygen gas collected, we use the equation given by ideal gas which follows:
where,
P = pressure of the gas = 732.2 torr
The conversion of P(torr) to P(atm) is shown below:
So,
Pressure = 732.2 / 760 atm = 0.9634 atm
V = Volume of the gas = 23 mL = 0.023 L
T = Temperature of the gas =
R = Gas constant =
n = number of moles of oxygen gas = ?
Applying the equation as:
0.9634 atm × 0.023 L = n × 0.0821 L.atm/K.mol × 295.15 K
⇒n = moles