I think this is what you're after:
Cs(g) → Cs^+ + e⁻ ΔHIP = 375.7 kJ mol^-1 [1]
Convert to J and divide by the Avogadro Const to give E in J per photon
E = 375700/6.022×10^23 = 6.239×10^-19 J
Plank relationship E = h×ν E in J ν = frequency (Hz s-1)
Planck constant h = 6.626×10^-34 J s
6.239×10^-19 = (6.626×10^-34)ν
ν = 9.42×10^14 s^-1 (Hz)
IP are usually given in ev Cs 3.894 eV
<span>E = 3.894×1.60×10^-19 = 6.230×10^-19 J per photon </span>
Because chemical energy is stored the chemical reaction takes place the stored chemical energy is released.
Answer:
Maybe try to memorize it by the valence electrons. You can do this!!
Answer: C. the same amount of energy as
Explanation:
A reversible reaction is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
Reversible reactions will reach an equilibrium point where the concentrations of the reactants and products will no longer change.
Thus if forward reaction is exothermic i.e. the heat is released , the backward reaction will be endothermic i.e. the heat is absorbed and in same amount.
The amount of energy released will be equal and opposite in sign to the energy absorbed in that reaction.
The total pressure in the container is <u>2.02</u> atm.
<em>Step</em> 1. Calculate the<em> total number of moles.
</em>
Moles of He = 1.00 g He × (1.00 mol He/4.003 g He) = 0.2498 mol He
Moles of F₂ = 14.0 g F₂ × (1 mol F₂/38.00 g F₂) = 0.3684 mol F₂
Moles of Ar = 19.00 g Ar × (1 mol Ar/39.95 g Ar) = 0.4756 mol Ar
<em>Total moles</em> = (0.2498 + 0.3684 + 0.4756) mol = <em>1.094 mol
</em>
<em>Step </em>2. Calculate the <em>total pressure</em>.
Use the <em>Ideal Gas Law</em>: <em>pV = nRT
</em>
We can solve the equation to get the pressure:
<em>p</em> = (<em>nRT</em>)/<em>V</em>
<em>n</em> = 1.094 mol
<em>R</em> = 0.082 06 L·atm·K⁻¹mol⁻¹
<em>T</em> = (20.0 + 273.15) K = 293.15 K
<em>V</em> = 13.0 L
∴ <em>p</em> = (1.094 mol × 0.082 06 L·atm·K⁻¹mol⁻¹ × 293.15 K)/13.0 L = 2.02 atm