The absorbance reported by the defective instrument was 0.3933.
Absorbance A = - log₁₀ T
Tm = transmittance measured by spectrophotometer
Tm = 0.44
Absorbance reported in this equipment = -log₁₀ (0.44) = 0.35654
True absorbance can be calculated by true transmittance, Tm = T+S(α-T)
S = fraction of stray light = 6%= 6/100 = 0.06
α= 1, ideal case
T = true transmittance of the sample
Tm = T+S(α-T)
now, T= Tm-S/ 1-S = 0.44-0.06/ 1-0.06 = 0.404233
therefore, actual reading measured is A = -log₁₀ T = -log₁₀ (0.404233)
i.e; 0.3933
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Answer:
Er-144 -------> Dy-140 + He-4
Explanation:
Alpha decay is the release of a hydrogen nucleus. So the original atom will decrease the mass by 4 and the atomic number by 2.
If we look at the periodic table, we see that phosphorous has an atomic mass of 30.97. Therefore, it has a molar mass of 30.97 g/mol. The answer is B.
Answer:
0.2990
Explanation:
All liquids intend to vaporize independent of the temperature if the pressure is higher enough. This pressure is called the vapor pressure. When it occurs, the liquid and the vapor phases will be in equilibrium, and so the fractions of the components of the liquids and the vapor can be calculated.
The molar fraction of the liquid (x) can be calculated by the composition, so, calling xc for cyclohexane, and ca for acetone:
xc = 1.90/(1.90 + 2.60) = 0.4222
xa = 1 - 0.4222 = 0.5778
The total pressure of the system (P) can be calculated by Dalton's Law:
P = Pc + Pa
Where Pc and Pa are the partial pressures of the components. The partial pressures can be calculated by the Raoult's Law:
Pc = xc*P°c
Pa = xa*P°a
Where P° is the vapor pressure, so:
P = xc*P°c + xa*P°a
P = 0.4222*97.6 + 0.5778*229.5
P = 137.8 torr
The molar fraction at the vapor phase (y) is the partial pressure divided by the total pressure:
yc = Pc/P
yc = (xc*P°c)/P
yc = (0.4222*97.6)/137.8
yc = 0.2990
This is an example of sphere interaction of the biosphere, hydrosphere, and lithosphere.
