Answer:
12426torr
Explanation:
The following data were obtained from the question:
n = 0.63 mole
V = 750mL = 750/1000 = 0.75L
T = -35.6°C = -35.6 + 273 = 237.4K
R =0.082atm.L/Kmol
P =?
Using the ideal gas equation PV = nRT, the pressure can be obtained as follows:
PV = nRT
P = nRT/V
P = (0.63 x 0.082 x 237.4)/0.75
P = 16.35atm
Now let us convert this pressure (i.e 16.35atm) to a pressure in torr. This is illustrated below:
1atm = 760torr
16.35atm = 16.35 x 760 = 12426torr
Therefore, the pressure of the gas is 12426torr
Isotopes of an element have same atomic number (number of protons) but vary in the mass number (number of neutrons). The chemical reactivity of an element is not affected by the change in mass number. So, for stable isotopes of Oxygen, (Oxygen-16, Oxygen-17 and Oxygen-18) the biochemical pathway of oxygen breathed in during respiration remains unaffected even with different isotopes. Only the radioactive isotopes of oxygen when breathed in may cause serious health hazards as they emit radiations that may damage the internal organs in the body.
The light intensity. The transparency of the filter, the bandwidth of the filter,
Also the color temperature of light source
If 4 moles of P is used by 5 mole of O2
then....0.489 moles will be used by 5/4 × .489 = .611 moles of O2
so .611 moles
so if 4 moles of P is burnt , 1 mole of P4O10 is produced ....so for .489 moles...... .489/4=.122 moles !
so mass will be .122× 283.89 = 34.7 grams
so first ans is .611 moles and second is 34.7 grams !
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