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
For a proton, the charge is represented by +e
For an electron, the charge is represented by -e
The charge of an electron [e] is equal to the - 1.602 * 10^-19 Coulombs
For an ionized atom, the net charge is equal to the sum of charges in the proton and the electron in that atom.
From the question, we are told that, the iron atom has 26 protons and 7 electrons.
The net charge Q = 26 [ +e] + 7 [- e] = +19 e
+19 e = + 19 [1.602 * 10^-19 C] = + 3.04 * 10^-18 C.
The correct answer is
C.
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Answer:
The molecular weight of the unknown gas is 16.1 g/mol.
When the solution is pure water so,
Kw = [OH-][H3O+]
when [OH-] = [H3O+] we can assume both = X
and Kw = 1.47 x 10^-14
by substitution:
1.47 x 10^-14 = X^2
∴ X = √(1.47 x 10^-14)
= 1.2 x 10^-7 M