The relationship between energy of a single photon and its wavelength can be determined using the formula E=hc/lambda where E is energy, h is Planck's constant, c is the speed of light, and lambda is photons.
Before being able to solve for energy, need to convert nanometers to meters.
407 nm (1 m/1 x 10^9 nm) = 4.07 x 10^-7 m
Then plug in the values we know into the equation.
E h(Planck's constant) c(speed of light)
E = (6.63 x 10^-34 Js)(3 x 10^8 m/s) / 4.07 x 10^-7 m (lambda)
E=(0.000000000000000000000000000000000663js)(300,000,000m/s)=1.989×10^-25j/ms
E=1.989x10^-25j/ms /{divided by} 4.07x10^-7m = 4.8869779x10^-33 J (the meters cancel out)
E = 4.89 x 10^-33 J
This gives us the energy in Joules of a single photon. Now, we can find the number of photons in 0.897 J
0.897J / 4.89 x 10^-33 J = ((0.897 J) / 4.89) x ((10^(-33)) J) = 1.8343558 x 10^-34
1.83435583 × 10-34m4 kg2 / s4 photons
this is a lot sorry i can't help
Answer:
455.4 g
Explanation:
Data given:
no. of moles of (NH₄)₂SO₄= 3.45 mol
mass of (NH₄)₂SO₄ = ?
Solution
Formula will be used
no.of moles = mass in grams / molar mass
Rearrange the above equation for mass
mass in grams = no. of moles x molar mass . . . . . . . . (1)
molar mass of (NH₄)₂SO₄
molar mass of (NH₄)₂SO₄ = 2(14 + 4(1)) + 32 + 4(16)
molar mass of (NH₄)₂SO₄ = 2 (14 +4) + 32 + 64
molar mass of (NH₄)₂SO₄ = 2 (18) + 32 + 64
molar mass of (NH₄)₂SO₄ = 36 + 32 + 64 = 132 g/mol
Put values in equation 1
mass in grams = 3.45 mole x 132 g/mol
mass in grams = 455.4 g
So,
mass of (NH₄)₂SO₄ = 455.4 g
Answer:
She overcame her disabilities to compete in the 1956 Summer Olympic Games, and in 1960, she became the first American woman to win three gold medals in track and field at a single Olympics. Later in life, she formed the Wilma Rudolph Foundation to promote amateur athletics.
Explanation:
