Answer:
final concentration: Ca = 0.014 M
Explanation:
Velocity of reaction:
∴ α: order of reaction, assuming α = 1
∴ K = 0.249 s-1.......rate constant
∴ Cao = 0.050 M......initial concentration
∴ t = 5 s.......reaction time
⇒ δCa/δt = K*Ca
⇒ ∫δCa/Ca = K*∫δt
⇒ Ln(Cao/Ca) = K*t = (0.249s-1)(5 s) = 1.245
⇒ Cao/Ca = 3.473
⇒ Ca = 0.050/3.473
⇒ Ca = 0.014 M
Answer:
12.4×10^3 V
Explanation:
From E=hc/wavelength= eV
The voltage becomes
V= hc/e* wavelength
V= 6.63*10^-34*3*10^8/1.6*10^-19*1*10^-10
Note that the energy of the photon is transferred to the electron. That is the basic assumption we have applied in solving this problem. The kinetic energy of the electron is equal to the product of the electron charge and the acceleration potential.
steps...
1) convert mass H2O to moles H2O
2) use coefficients of balanced equation to convert to moles O2
3) convert moles O2 to L O2.
solution...
10.5 g H2O x (1 mole H2O / 18.0 g H2O) = 0.583 moles H2O
from the balanced equation, 1 mole O2 --> 2 moles H2O.. therefore...
0.583 moles H2O x (1 mole O2 / 2 moles H2O) = 0.292 moles O2
from here you can either use the specific form of the ideal gas law for STP...
0.292 moles O2 x (22.4 L O2 / mole O2) = 6.54 L O2
or you can use the more general form of the ideal gas law...
V = nRT/P = (0.292 moles) x (0.0821 Latm/moleK) x (273 K) / (1 atm)
V = 6.54 L O2
Hope this helps!
The ionization reaction of the compound given are as follows:
1.) HI(aq)
HI(aq) -----> H+(aq) + I-(aq)
2.) LiOH(s)
LiOH(s) ------> Li+(aq) + OH-(aq)
Ionization<span> is the process by which an atom or a molecule acquires a negative or positive charge. Hope this helps. Have a nice day.</span>
