Answer:
P₂ = 5.550213 Pa
Explanation:
Given data:
Heat of vaporization = 376.6 KJ/mol ( 376600 j/mol)
R = 8.3143 j mol⁻¹ K⁻¹
Temperature = T1 = 100 °C = 100 + 273 = 373 K
Temperature = T2 = 508.0 °C = 508.0+273 = 781 K
Pressure at 100°C= P1 = 1.6 × 10⁻³² Pa
Pressure at 508.0 °C = ?
Solution:
ln P₁/P₂ = ΔH /R ( 1/T₂ - 1/T₁)
ln (1.6 × 10⁻³² Pa) - ln (P₂) = 376600 j. mol⁻¹ / 8.3143 j mol⁻¹ K⁻¹ ( 1/T₂ - 1/T₁)
-73.212719 - ln (P₂) = 45295.45 (0.001280 - 0.002680)
-73.212719 - ln (P₂) = 45295.45 (-0.00414)
- ln (P₂) = -63.41363 + 73.212719
- ln (P₂) = 9.799089
P₂ = e⁻⁹°⁷⁹⁹⁰⁸⁹
P₂ = 5.550213 Pa
Per ml, aluminum has 2.7 grams of mass. So in 250 ml, there are (2.7)*(250) number of grams.
675 grams.
Ans: 7 electrons
The peaks in a photoelectron spectrum correspond to the binding energy of electrons in a given substance. The lower energy peaks represent the binding energy of the outer or valence electrons whereas the higher energy peaks correspond to that of the inner and core electrons.
The atomic number of bromine is 35. The electron configuration would be:
Br[35] =[ 1s²2s²2p⁶3s²3p⁶3d¹⁰]4s²4p⁵
The valence electron configuration is:
Br[35] = 4s²4p⁵
there are 7 valence electrons, thus the lowest energy peak would be associated with 7 electrons.
C = 12.818 mg CO2 (1 mmol CO2/44 mg CO2) (1 mmol C/1 mmol
CO2) = 0.29 mmol
H = 3.675 mg of H2O (1 mmol H2O/18 mg H2O) (2 mmol H/1
mmol H2O) = 0.41 mmol
N = (4.725 mg – 0.29 * 12 – 0.41 * 1) * (1 mmol/14 mg) =
0.06 mmol
Divide everything by the smallest number:
C = 0.29/0.06 = 4.8 ~ 5
<span>H = 0.41/0.06 = 6.8 ~
7</span>
N = 0.06/0.06 = 1
Empirical formula is:
<span>C5H7N</span>
To know the answer to this problem, you can search online or in any textbooks for the chemical formula of quinine. This is essential because you can detect from the chemical formula the number of hydrogen atoms.
Quinine has the chemical formula C₂₀H₂₄N₂O₂. So, the ratio of hydrogen to quinine is 24/1.
<em>Moles of hydrogen = 1.1 mol quinine * 24/1 = 26.4 mol</em>