This problem is to use the Claussius-Clapeyron Equation, which is:
ln [p2 / p1] = ΔH/R [1/T2 - 1/T1]
Where p2 and p1 and vapor pressure at estates 2 and 1
ΔH is the enthalpy of vaporization
R is the universal constant of gases = 8.314 J / mol*K
T2 and T1 are the temperatures at the estates 2 and 1.
The normal boiling point => 1 atm (the pressure of the atmosphere at sea level) = 101,325 kPa
Then p2 = 101.325 kPa
T2 = ?
p1 = 54.0 kPa
T1 = 57.8 °C + 273.15K = 330.95 K
ΔH = 33.05 kJ/mol = 33,050 J/mol
=> ln [101.325/54.0] = [ (33,050 J/mol) / (8.314 J/mol*K) ] * [1/x - 1/330.95]
=> 0.629349 = 3975.22 [1/x - 1/330.95] = > 1/x = 0.000157 + 1/330.95 = 0.003179
=> x = 314.6 K => 314.6 - 273.15 = 41.5°C
Answer: 41.5 °C
Answer:
There is two iron atoms.
Explanation:
The formula iron oxide is Fe2O3 F e 2 O 3 therefore there would be two. Hope this helps. :)
Answer:
Is better use the Benedict's test by the increase in the amount of the products if the enzyme is a reductase
Explanation:
The Benedict's test works by the reaction of the reducing sugars with the ion cupric of the reactive. If the enzyme is a reductase (degrades polysaccharides into bi o monosaccharides), it should cut the polysaccharide bond and the products would react with the Benedict's cupric ion
I hope you undestand me
Answer:
89.6 liters
Explanation:
A STP (standard temperature and pressure) ONE mole of any idea gas will occupies 22.4 liters. So,...
4 moles x 22.4 L/mol = 89.6 liters
Answer:
Primero debes usar los gramos de co2 y luego buscar su peso molecular, luego de eso usar la relación de moles entre CO2 y H2O y por último buscar el pm del H2O pata ver cuantos gramos de produce.
Explanation:
