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REY [17]
3 years ago
15

A light ray traveling through a material with an index of refraction of 1.2 is incident on a material that has an index of refra

ction of 1.4. Compared to the incident angle, the refracted angle of the light ray is
Physics
1 answer:
zzz [600]3 years ago
3 0

Answer:

compared to the incident angle, the refracted angle is 45.56⁰

Explanation:

From Snell's law;

n₁sin(I) = n₂sin(r)

Where;

n₁ is the refractive index of light in medium 1 = 1.2

n₂ is the refractive index of light in medium 2 = 1.4

I is the incident angle

r is the refractive angle

n = \frac{1}{sin(I)}\\\\sin(I) = \frac{1}{n}\\\\sin(I) =\frac{1}{1.2}\\\\sin(I) =0.8333\\\\I = sin^-{(0.8333)

I = 56.439⁰

Applying snell's law

n_1sin(I) = n_2sin(r)\\\\sin(r) = \frac{n_1sin(I) }{n_2}\\\\sin(r) = \frac{1.2*sin(56.439) }{1.4}\\\\sin(r) = 0.714\\\\r = sin^-(0.714)\\\\r = 45.56^o

Therefore, compared to the incident angle, the refracted angle is 45.56⁰

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3 years ago
A circular room has a radius of 3.0 m. An 80 kg man stands with his back against the wall. The room then spins so the man is mov
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Answer:

Explanation:

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Centripetal force, Fc = M × v^2/R

Fc = N

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4 years ago
A mass of 0.1 kg of helium fills a 0.2 m3 rigid tank at 350 kPa. The vessel is heated until the pressure is 700 kPa. Calculate t
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Explanation:

(a)   First, we will calculate the number of moles as follows.

       No. of moles = \frac{\text{mass}}{\text{molar mass}}

Molar mass of helium is 4 g/mol and mass is given as 0.1 kg or 100 g (as 1 kg = 1000 g).

Putting the given values into the above formula as follows.

       No. of moles = \frac{\text{mass}}{\text{molar mass}}

                             = \frac{\text{100 g}}{4 g/mol}  

                             = 25 mol

According to the ideal gas equation,

                           PV = nRT

or,       (P_{2} - P_{1})V = nR (T_{2} - T_{1})

          (6.90 atm - 3.45 atm) \times 200 L = 25 \times 0.0821 L atm/mol K \Delta T

          \Delta T = 336.17 K

Hence, temperature change will be 336.17 K.

(b)   The total amount of heat required for this process will be calculated as follows.

                   q = mC \Delta T

                      = 100 g \times 5.193 J/g K \times 336.17 K

                      = 174573.081 J/K

or,                  = 174.57 kJ/K        (as 1 kJ = 1000 J)

Therefore, the amount of total heat required is 174.57 kJ/K.

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