The oxidation numbers of nitrogen in NH3, HNO3, and NO2 are, respectively: -3, -5, +4 +3, +5, +4 -3, +5, -4 -3, +5, +4
Evgesh-ka [11]
In NH3 , let oxidation number of N be x
x + (+1)3 = 0
x = -3
In HNO3 , let oxidation number of N be x
1 + x + (-2)3 = 0
x = +5
In NO2 , let oxidation number of N be x
x + (-2)2 = 0
x = +4
Answer:
c
Explanation:
hypothesis is a scientific guess made be scientist in order to give account for the natural phenomenon
The diatomic molecule that is formed when two atoms share six electrons is N2.
The atomic number of nitrogen is 7 and its electronic configuration is 2,5. This implies that, nitrogen has 5 electrons in its outermost shell. To attain the octet structure, it needs 3 electrons more. To form a diatomic molecule, two nitrogen atoms come together and each donate three electrons, which are equally shared between the two, thus, each ends up having 8 electrons in its outermost shell.
Answer:
The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.
Explanation:
It takes 839 kJ/mol to break a carbon-carbon triple bond.
Energy required to break 1 mole of carbon-carbon triple bond = E = 839 kJ
E = 839 kJ/mol = 839,000 J/mol
Energy required to break 1 carbon-carbon triple bond = E'
The energy require to single carbon-carbon triple bond will corresponds to wavelength which is required to break the bond.
(Using planks equation)
The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.
<h3>Answer:</h3>
0.8133 mol
<h3>Solution:</h3>
Data Given:
Moles = n = ??
Temperature = T = 25 °C + 273.15 = 298.15 K
Pressure = P = 96.8 kPa = 0.955 atm
Volume = V = 20.0 L
Formula Used:
Let's assume that the Argon gas is acting as an Ideal gas, then according to Ideal Gas Equation,
P V = n R T
where; R = Universal Gas Constant = 0.082057 atm.L.mol⁻¹.K⁻¹
Solving Equation for n,
n = P V / R T
Putting Values,
n = (0.955 atm × 20.0 L) ÷ (0.082057 atm.L.mol⁻¹.K⁻¹ × 298.15 K)
n = 0.8133 mol
