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pickupchik [31]
3 years ago
9

A battery is connected at its positive end by a wire to the head of an iron nail. The wire then coils aground the nail to its ti

p and from there to the negative end of the battery.
Predict what would happen to the strength of the electromagnet in each situation.
Using a battery with a higher voltage:
Wrapping the wire around the nail only three times:
Changing the direction of the current by reversing the battery connections:
Using a plastic stick in place of the iron nail:
Holding the nail vertically rather than horizontally: it
Chemistry
2 answers:
cupoosta [38]3 years ago
7 0

Answer:

sing a battery with a higher voltage:  

✔ stronger force of attraction

Wrapping the wire around the nail only three times:  

✔ weaker force of attraction

Changing the direction of the current by reversing the battery connections:  

✔ no change

Using a plastic stick in place of the iron nail:  

✔ weaker force of attraction

Holding the nail vertically rather than horizontally:  

✔ no change

Explanation: You're Welcome

puteri [66]3 years ago
7 0

Answer:

✔ stronger force of attraction

✔ weaker force of attraction

✔ no change

✔ weaker force of attraction

✔ no change

Explanation:

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  • <u><em>Sodium chloride</em></u>
  • See the graph attached

Explanation:

The attached graph with a green and a red arrow facilitates the understanding of this explanation.

To read the <em>solubility </em>on the <em>graph</em>, you can start with the temperature, on the x-axis.

The red vertical arrow shows how, departing from the <em>40ºC temperature</em> on the x-axis, you intersect the<em> solutibility curve </em>of sodium chloride at a height (y-axis) corresponding to <em>60 g/100cm³ of water</em> (follow the green horizontal arrow).

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A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 4250 mL of water at 2
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Answer:

The specific heat of copper is 0.385 J/g°C

Explanation:

A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 425 mL of water at 22.55 degrees Celsius. The final temperature of the water was recorded to be 26.15 degrees Celsius. What is the specific heat of the copper?

Step 1: Data given

Mass of copper = 85.2 grams

Temperature of copper = 221.32 °C

Volume of water = 425 mL

Temperature of water = 22.55 °C

Final temperature = 26.15 °C

Specific heat of water = 4.184 J/g°C

Step 2: Calculat the specific heat of copper

Heat lost = heat gained

Q = m*c*ΔT

Qcopper = -Qwater

m(copper)*c(copper)*ΔT(copper) = - m(water) * c(water) * ΔT(water)

⇒ m(copper) = 85.2 grams

⇒ c(copper) = TO BE DETERMINED

⇒ ΔT(copper) = the change in temeprature = T2 -T1 = 26.15 -221.32 = -195.17 °C

⇒ m(water) = The mass of water = 425 mL * 1g/mL = 425 grams

⇒ c(water) = The specific heat of water = 4.184 J/g°C

⇒ ΔT(water) = The change of temperature of water = 26.15 - 22.55 = 3.6

85.2 * c(copper) * (-195.17) = -425 * 4.184 * 3.6

c(copper) = 0.385 J/g°C

The specific heat of copper is 0.385 J/g°C

(Note, The original question says the volume of the water is 4250 mL. IF this is not an error, the specific heat of copper is 3.85 J/g°C (10x higher than the normal value).

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In this case the number of protons 39 (atomic number 39) permit you to identify the element as gallium.

Now, to identify the isotope you tell the name of the element and add the mass number.

The mass number is the sum of the protons and the neutrons

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Therefore, the isotope is gallium - 72.

Answer: isotope gallium - 72

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