Answer:
The pressure of O₂ is 0.8 atm.
Explanation:
The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:
PT = PA + PB
This relationship is due to the assumption that there are no attractive forces between the gases.
In this case:
PT=Pnitrogen + Pcarbon dioxide + Pother gases
Being:
- Pnitrogen: 593.4 mmHg
- Pcarbon dioxide: 3 mmHg
- Pother gases: 7.1 mmHg
and replacing:
PT= 593.4 mmHg + 3 mmHg + 7.1 mmHg
you get:
PT= 603.5 mmHg
Being 760 mmHg= 1 atm, you get:
PT= 603.5 mmHg= 0.8 atm
<u><em>The pressure of O₂ is 0.8 atm.</em></u>
Hey there!:
Isotopes : abundance :
46 Ti 8.0%
47 Ti 7.8 %
48 Ti 73.4 %
49 Ti 5.5 %
50 Ti 5.3 %
Weighted average = ∑ Wa * % / 100
Therefore:
( 46 * 8.0) + (47 * 7.8 ) + (48 * 73.4 ) + ( 49 * 5.5 ) + ( 50*5.3 ) / 100 =
4792.3 / 100
= 47.923 a.m.u
Hope that helps!
The balanced equation for the reaction is as follows;
Ca(OH)₂ + 2HBr --> CaBr₂ + 2H₂O
stoichiometry of Ca(OH)₂ to HBr is 1:2
number of Ca(OH)₂ moles reacted - 0.10 mol/L x 0.1000 L = 0.010 mol
Number of HBr moles added - 0.10 mol/L x 0.4000 = 0.040 mol
1 mol of Ca(OH)₂ needs 2 mol of HBr for neutralisation
therefore 0.010 mol of Ca(OH)₂ needs - 0.010 x 2 = 0.020 mol of HBr to be neutralised
but 0.040 mol of HBr has been added therefore number of moles of HBr in excess - 0.040 - 0.020 = 0.020 mol
then pH of the medium can be calculated using the excess H⁺ ions
HBr is a strong acid therefore complete ionization
[HBr] = [H⁺]
[H⁺] = 0.020 mol / (100.0 + 400.0 mL)
= 0.020 mol / 0.5 L
= 0.040 mol/L
pH = -log[H⁺]
pH = - log [0.040 M]
pH = 1.40
pH of the medium is 1.40
Answer:
Explanation:
Given that,
The wavelength of a microwave is 7.42 mm or 0.00742 m
No. of photons, n = 359
We need to find the energy produced by this no of photons. It can be given by the formula as follows :
or
So, the required energy is 
.
