Answer:
The law is given by the following equation: PV = nRT, where P = pressure, V = volume, n = number of moles, R is the universal gas constant, which equals 0.0821 L-atm / mole-K, and T is the temperature in Kelvin.
Explanation:
Answer:
a) 1.269 × 10^-7 m
b) This wavelength occurs in the ultraviolet region of the electromagnetic spectrum
Explanation:
The energy required to break the bond= energy of the incident photon
E= 941 × 10^3/6.02 × 10^23 = 1.56 ×10^ -18 J
From
E= hc/λ
h= Plank's constant
c= speed of light
λ= wavelength of incident photon
λ= hc/E
λ= 6.6 ×10^-34 × 3 ×10^8/1.56 ×10^ -18 J
λ= 1.269 × 10^-7 m
b) This wavelength occurs in the ultraviolet region of the electromagnetic spectrum
The answer for this question is niche.
The molar volume of a gas at STP occupies <u>22.4 L.</u>
Option D
<u>Explanation:</u>
To find the volume of 1 mole of a gas at STP, we use the Ideal Gas Law. It is the general gas equation which gives the relation to the measurable quantities to an ideal gas as below,
P (pressure) × V (volume) = n (number of moles) × R (the gas constant) × T (temperature in Kelvin)
STP = 1 atm of pressure and 273 K for temperature
P = 1 atm
V = ?
n = 1 mole
R = 0.0821 atm L/mol K
T = 273 K
Using the equation,
![\mathrm{PV}=\mathrm{nRT}](https://tex.z-dn.net/?f=%5Cmathrm%7BPV%7D%3D%5Cmathrm%7BnRT%7D)
![V=\frac{n R T}{P}](https://tex.z-dn.net/?f=V%3D%5Cfrac%7Bn%20R%20T%7D%7BP%7D)
By substituting the above values, in the equation,
![V=\frac{1 \times 0.082 \times 273}{1}=22.38\ L](https://tex.z-dn.net/?f=V%3D%5Cfrac%7B1%20%5Ctimes%200.082%20%5Ctimes%20273%7D%7B1%7D%3D22.38%5C%20L)
V = 22.38 L