Answer:
Answers. 7.8286×10²¹ particles.
Explanation:
The correct answer to this question is this one:
find the energy of one photon:
<span>E=h*<span>c/λ
</span></span>
divide the energy given by the energy of one photon of that wavelength
What I've done so far is convert wave length to m and energy to j.
E photon = h * x / wave length
E = (6.626 x 10^-43)(3.00 x 10^8) / 587 ^ -9 = 3.38 x 10 ^18 J
3.38 x 10 ^18 J x 1000 kj / 1 j = 3.37 x 10 ^ 16 Kj
609 kJ/ 3.37 x 10 ^ 16 Kj = 1.81 x 10 ^ 16
E = (6.626 x 10^-34)(3.00 x 10^8) / 587 ^ -9 = 3.38 x 10 ^19 J
3.38 x 10 ^19 J x 1000 kj / 1 j = 3.37 x 10 ^ -16 Kj
609 kJ/ 3.37 x 10 ^ 16 Kj = 1.81 x 10 ^ 18 but the answer is 1.81 × 10^24 photons
3.38 x 10 ^-19 J
should be negative
then 3.38 x 10 ^18 J x 1kJ/1000 J
you're converting from J to kJ.. just like meters to kilometres, you wouldn't multiply you would divide
Answer:
young plains called maria and are composed of basalt
Explanation:
Answer: The theoretical yield and percent yield for this experiment are 40 g and 82% respectively.
Explanation:
![2KClO_3\rightarrow 2KCl+3O_2](https://tex.z-dn.net/?f=2KClO_3%5Crightarrow%202KCl%2B3O_2)
According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number
of particles.
To calculate the moles:
![\text{Moles of potassium chloride}=\frac{\text{Mass of potassium chloride}}{\text{Molar mass of potassium chloride}}=\frac{33g}{74.5g/mole}=0.44moles](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20potassium%20chloride%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20potassium%20chloride%7D%7D%7B%5Ctext%7BMolar%20mass%20of%20potassium%20chloride%7D%7D%3D%5Cfrac%7B33g%7D%7B74.5g%2Fmole%7D%3D0.44moles)
![\text{Moles of potassium chlorate}=\frac{\text{Mass of potassium chlorate}}{\text{Molar mass of potassium chlorate}}=\frac{66g}{122.5g/mole}=0.54moles](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20potassium%20chlorate%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20potassium%20chlorate%7D%7D%7B%5Ctext%7BMolar%20mass%20of%20potassium%20chlorate%7D%7D%3D%5Cfrac%7B66g%7D%7B122.5g%2Fmole%7D%3D0.54moles)
According to stochiometry:
2 moles of
produce = 2 moles of ![KCl](https://tex.z-dn.net/?f=KCl)
0.54 moles of
should produce =
of ![KCl](https://tex.z-dn.net/?f=KCl)
Thus theoretical yield is ![moles\times {\text {Molar mass}}=0.54mol\times 74.5g/mol=40g](https://tex.z-dn.net/?f=moles%5Ctimes%20%7B%5Ctext%20%7BMolar%20mass%7D%7D%3D0.54mol%5Ctimes%2074.5g%2Fmol%3D40g)
But Experimental yield is 33 g.
![{\text {percentage yield}}=\frac{\text {Experimental yield}}{\text {Theoretical yield}}\times 100\%](https://tex.z-dn.net/?f=%7B%5Ctext%20%7Bpercentage%20yield%7D%7D%3D%5Cfrac%7B%5Ctext%20%7BExperimental%20yield%7D%7D%7B%5Ctext%20%7BTheoretical%20yield%7D%7D%5Ctimes%20100%5C%25)
![{\text {percentage yield}}=\frac{33g}{40g}\times 100\%=82\%](https://tex.z-dn.net/?f=%7B%5Ctext%20%7Bpercentage%20yield%7D%7D%3D%5Cfrac%7B33g%7D%7B40g%7D%5Ctimes%20100%5C%25%3D82%5C%25)
The theoretical yield and percent yield for this experiment are 40 g and 82% respectively.