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Oxana [17]
4 years ago
5

In a classroom demonstration, two long parallel wires are separated by a distance of 2.25 cm. One wire carries a current of 1.30

A while the other carries a current of 3.15 A. The currents are in the same direction. (a) What is the magnitude of the force per unit length (in N/m) that one wire exerts on the other
Physics
1 answer:
Dafna11 [192]4 years ago
4 0

Answer:

Explanation:

Given that,

Current in wire are 1.3A and 3.15A

Distance between wire is d= 2.25cm

d = 2.25/100 = 0.025m

Force per unit length F/l?

Let us consider the field produced by wire 1 and the force it exerts on wire 2 (call the force F2).

The field due to I1 at a distance r is given to be

B1 = μo• I1 / 2πr

This field is uniform along wire 2 and perpendicular to it, and so the force F2 it exerts on wire 2 is given by

F=ILBsinθ

with sinθ=1:

F2=I2 • L •B1

By Newton’s third law, the forces on the wires are equal in magnitude, and so we just write F for the magnitude of F2. (Note that F1=−F2.) Since the wires are very long, it is convenient to think in terms of F/l, the force per unit length. Substituting the expression for B1 into the last equation and rearranging terms gives

F/l = μo• I1• I2 / 2πr

Where μo is constant

μo = 4π×10^7 Tm/A

Then,

F/l = μo• I1• I2 / 2πr

F/l = 4π ×10^-7 × 1.3×3.15/(2π×0.025)

F/l = 3.276×10^-5 N/m

the magnitude of the force per unit length that one wire exerts on the other is 3.276×10^-5 N/m

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3 years ago
A gas mixture contains 320mg methane, 175 mg argon, 225 mg nitrogen (N2). The partial pressure of argon at 300K is 12.52 kPa. Wh
svet-max [94.6K]

<u>Answer:</u> The volume and total pressure of the mixture is 0.876 L and 89.36 kPa respectively.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

  • <u>For methane:</u>

Given mass of methane = 320 mg = 0.3 g     (Conversion factor:  1 g = 1000 mg)

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

\text{Moles of methane}=\frac{0.3g}{16g/mol}=0.019mol

  • <u>For argon:</u>

Given mass of argon = 175 mg = 0.175 g

Molar mass of argon = 40 g/mol

Putting values in equation 1, we get:

\text{Moles of argon}=\frac{0.175g}{40g/mol}=0.0044mol

  • <u>For nitrogen:</u>

Given mass of nitrogen = 225 mg = 0.225 g

Molar mass of nitrogen = 28 g/mol

Putting values in equation 1, we get:

\text{Moles of nitrogen}=\frac{0.225g}{28g/mol}=0.0080mol

To calculate the volume of the mixture, we use the equation:

PV = nRT         ......(2)

We are given:

Partial pressure of argon = 12.52 kPa

Temperature = 300 K

R = Gas constant = 8.31\text{L kPa }mol^{-1}K^{-1}

n = number of moles of argon = 0.0044 moles

Putting values in equation 2, we get:

12.52kPa\times V=0.0044mol\times 8.31\text{L kPa }mol^{-1}K^{-1}\times 300K\\\\V=\frac{0.0044\times 8.31\times 300}{12.52}=0.876L

Now, calculating the total pressure of the mixture by using equation 2:

Total number of moles = [0.019 + 0.0044 + 0.0080] mol = 0.0314 mol

V= volume of the mixture = 0.876 L

Putting values in equation 2, we get:

P\times 0.876L=0.0314mol\times 8.31\text{L kPa }mol^{-1}K^{-1}\times 300K\\\\P=\frac{0.0341\times 8.31\times 300}{0.876}=89.36kPa

Hence, the volume and total pressure of the mixture is 0.876 L and 89.36 kPa respectively.

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