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3 years ago

An atom does not need any electrons if it has _____ outermost shell

Chemistry

1 answer:

Andreyy893 years ago

6 0

Atom does not need any electrons if it has a completely filled outermost shell.

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A 15.0 g sample of nickel metal is heated to 100.0 degrees C and dropped into 55.0 g of water, initially at 23.0 degrees C. Assu

OLEGan [10]

Answer: The final temperature of nickel and water is $25.2^{o}C$ .

Explanation:

The given data is as follows.

Mass of water, m = 55.0 g,

Initial temp, $(t_{i}) = 23^{o}C$ ,

Final temp, $(t_{f})$ = ?,

Specific heat of water = 4.184 $J/g^{o}C$ ,

Now, we will calculate the heat energy as follows.

q = $mS \Delta t$

= $55.0 g \times 4.184 J/g^{o}C \times (t_{f} - 23^{o}C)$

Also,

mass of Ni, m = 15.0 g,

Initial temperature, $t_{i} = 100^{o}C$ ,

Final temperature, $t_{f}$ = ?

Specific heat of nickel = 0.444 $J/g^{o}C$

Hence, we will calculate the heat energy as follows.

q = $mS \Delta t$

= $15.0 g \times 0.444 J/g^{o}C \times (t_{f} - 100^{o}C)$

Therefore, heat energy lost by the alloy is equal to the heat energy gained by the water.

$q_{water}(gain) = -q_{alloy}(lost)$

$55.0 g \times 4.184 J/g^{o}C \times (t_{f} - 23^{o}C)$ = -( $15.0 g \times 0.444 J/g^{o}C \times (t_{f} - 100^{o}C)$ )

$t_{f} = \frac{25.9^{o}C}{1.029}$

= $25.2^{o}C$

Thus, we can conclude that the final temperature of nickel and water is $25.2^{o}C$ .

6 0

3 years ago

James exclaims to his chemistry teacher that a new element has been discovered that fits between Nickel and Copper on the period

myrzilka [38]

Aye you have the same class as me bruh I need help on some chemistry qustions

8 0

3 years ago

Read 2 more answers

What is the molarity of a solution that is prepared by adding 3 moles of CaSO4 in 1.5 L of water?

blondinia [14]

Answer:

$[CaSO_4] = 2 mol/L$

Explanation:

$[CaSO_4] = \frac{3 mol}{1.5 L} = 2 mol/L$

6 0

2 years ago

What is the mass in grams of 1.50 X 1023 molecules of NaOH?

avanturin [10]

Answer:

a. 10.0 g

Explanation:

The molar mass of NaOH is 39.997 grams which was calculated by adding the molar mass of Sodium, Oxygen, and Hydrogen $22.990 + 15.999 + 1.008 = 39.997$ . But before we do anything with this number we must first convert $1.50 * 10^{23}$ molecules to moles. We can do this by dividing by Avogadro's number or $6.022*10^{23}$ ( $\frac{1.50*10^{23}}{6.022*10^{23}} = 0.24909$ moles). We then convert moles to grams by multiplying by the molar mass of NaOH, ( $0.24909 * 39.997 = 9.96$ grams). This is almost exactly 10 and the margin of error is likely due to the original numbers not being precise enough.

5 0

4 years ago

What type of reaction is shown by this equation?

Romashka-Z-Leto [24]

This is an acid base reaction which is basically a double displacement reaction. However, since carbonic acid is produced, it rapidly decomposes to carbon dioxide and water.

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3 years ago