Answer: n∗R=22+273.15/4.2∗5n
P2=n∗R∗T2/V2=n∗R∗33.6+273.15/10
Explanation:
Alpha helix and beta sheets are the secondary structure of protein
Answer:
a) +640 kJ/mol or +1.06x10⁻¹⁸ J
b) +276 kJ/mol
Explanation:
To dissociate the molecule, the bond must be broken, thus, it's necessary energy equal to the energy of the bond, which can be calculated by:
E = (Q1*Q2)/(4*π*ε*r)
Where Q is the charge of the ions, ε is a constant (8.854x10⁻¹²C²J ⁻¹ m⁻¹), and r is the bond length. Each one of the ions has a charge equal to 1. The elementary charge is 1.602x10⁻¹⁹C, which will be the charge of them.
1 mol has 6.022x10²³ molecules (Avogadros' number), so the energy of 1 mol is the energy of 1 molecule multiplied by it:
E = 6.022x10²³ *(1.602x10⁻¹⁹)²/(4π*8.854x10⁻¹²*2.17x10⁻¹⁰)
E = +640113 J/mol
E = +640 kJ/mol
Or at 1 molecule: E =640/6.022x10²³ = +1.06x10⁻²¹ kJ = +1.06x10⁻¹⁸ J
b) The energy variation to dissociate the molecule at its neutral atoms is the energy of dissociation less the difference of the ionization energy of K and the electron affinity of F (EA):
498 = 640 - (418 - EA)
640 -418 + EA = 498
222 + EA = 498
EA = +276 kJ/mol
Answer: ![Rate=k[L]^1[M]^2](https://tex.z-dn.net/?f=Rate%3Dk%5BL%5D%5E1%5BM%5D%5E2)
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
![Rate=k[L]^x[M]^y](https://tex.z-dn.net/?f=Rate%3Dk%5BL%5D%5Ex%5BM%5D%5Ey)
(1)
k= rate constant
x = order with respect to L
y = order with respect to M
n =( x+y)= Total order
a) If [L] is doubled, the reaction rate will increase by a factor of 2:
![2\times Rate=k[2L]^x[M]^y](https://tex.z-dn.net/?f=2%5Ctimes%20Rate%3Dk%5B2L%5D%5Ex%5BM%5D%5Ey)
(2)
b) If [M] is doubled, the reaction rate will increase by a factor of 4:
![4\times Rate=k[L]^x[2M]^y](https://tex.z-dn.net/?f=4%5Ctimes%20Rate%3Dk%5BL%5D%5Ex%5B2M%5D%5Ey)
(3)
Dividing 2 by 1:
![\frac{2\times Rate}{Rate}=\frac{k[2L]^x[M]^y}{k[L]^x[M]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B2%5Ctimes%20Rate%7D%7BRate%7D%3D%5Cfrac%7Bk%5B2L%5D%5Ex%5BM%5D%5Ey%7D%7Bk%5BL%5D%5Ex%5BM%5D%5Ey%7D)
Dividing 3 by 1
![\frac{4\times Rate}{Rate}=\frac{k[L]^x[2M]^y}{k[L]^x[M]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B4%5Ctimes%20Rate%7D%7BRate%7D%3D%5Cfrac%7Bk%5BL%5D%5Ex%5B2M%5D%5Ey%7D%7Bk%5BL%5D%5Ex%5BM%5D%5Ey%7D)
Thus rate law is: ![k[L]^1[M]^2](https://tex.z-dn.net/?f=k%5BL%5D%5E1%5BM%5D%5E2)
