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Nitella [24]
4 years ago
5

What is the emf produced in a 1.5 meter wire moving at a speed of 6.2 meters/second perpendicular to a magnetic field of strengt

h 3.96 × 10-3 newtons/amp·meter ?
a.37 volts
b.0.0026 volts
c.5.0 volts
d.0.37 volts
e.0.037 volts
Chemistry
2 answers:
My name is Ann [436]4 years ago
5 0

Answer : The correct option is, (e) 0.037 volts

Explanation :

Induced EMF formula :

e=Blv

where,

e = emf

B = magnetic field = 3.96\times 10^{-3}Newtons/amp.meter

l = length of the conductor = 1.5 meter

v = speed of the conductor = 6.2 meter/second

Now put all the given values in the above formula, we get the emf.

e=(3.96\times 10^{-3})\times (1.5)\times (6.2)=0.037V

Therefore, the emf is, 0.037 volts

Cerrena [4.2K]4 years ago
4 0
Hello there.

Question: <span>What is the emf produced in a 1.5 meter wire moving at a speed of 6.2 meters/second perpendicular to a magnetic field of strength 3.96 × 10-3 newtons/amp·meter ?

a.37 volts
b.0.0026 volts
c.5.0 volts
d.0.37 volts
e.0.037 volts

Answer: It would be E. 0.037.

Hope This Helps You!
Good Luck Studying ^-^</span>
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A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500 ml of solution. what is the calcium ion concentration in thi
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First calculate the number of moles of CaBr2 given the molar mass of 199.89 g/mol.

moles CaBr2 = 0.9182 g / (199.89 g / mol) = 4.60 x 10^-3 mol

 

We see that each CaBr2 contains only 1 mole of Ca, so the moles of Ca is also:

moles Ca+ = 4.60 x 10^-3 mol

 

So the molarity of this is:

Molarity Ca+ = 4.60 x 10^-3 mol / 0.500 L

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Answer:

TIMED HELP ASAP

19.11 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g・°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.

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You are running a rather large scale reaction where you prepare the grignard reagent phenylmagnesium bromide by reacting 210.14
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Answer:

We would expect to form 7.35 moles of grignard reagent.

Explanation:

<u>Step 1: </u>Data given

Mass of magnesium = 210.14 grams

Volume bromobenzene = 772 mL

Density of bromobenzene = 1.495 g/mL

Molar mass of Mg = 24.3 g/mol

Molar mass of bromobenzene = 157.01 g/mol

<u>Step 2</u>: The balanced equation

C6H5Br + Mg ⇒ C6H5MgBr

<u>Step 3:</u> Calculate mass of bromobenzene

Mass bromobenzene = density bromobenzene * volume

Mass bromobenzene = 1.495 g/mL * 772 mL

Mass bromobenzene = 1154.14 grams

<u>Step 4</u>: Calculate number of moles bromobenzene

Moles bromobenzene = mass bromobenzene / molar mass bromobenzene

Moles bromobenzene = 1154.14g / 157.01 g/mol

Moles bromobenzene = 7.35 moles

<u>Step 5:</u> Calculate moles of Mg

Moles Mg = 210.14 grams /24.3 g/mol

Moles Mg = 8.65 moles

<u>Step 6:</u> The limiting reactant

The mole ratio is 1:1 So the bromobenzene has the smallest amount of moles, so it's the limiting reactant. It will be completely consumed ( 7.35 moles). Magnesium is in excess, There will react 7.35 moles. There will remain 8.65 - 7.35 = 1.30 moles

<u>Step 7:</u> Calculate moles of phenylmagnesium bromide

For 1 mole of bromobenzene, we need 1 mole of Mg to produce 1 mole of phenylmagnesium bromide

For 7.35 moles bromobenzene, we have 7.35 moles phenylmagnesium bromide

We would expect to form 7.35 moles of grignard reagent.

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