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Akimi4 [234]
3 years ago
15

3.25*10^25 atoms of neon gas equals how many moles of neon gas?

Chemistry
2 answers:
gayaneshka [121]3 years ago
8 0

Answer:

53.97 moles

Explanation:

First off, it is important to understand the following concepts;

Avogadro's number is a proportion that relates molar mass on an atomic scale to physical mass on a human scale.

Avogadro's number is defined as the number of elementary particles (molecules, atoms, compounds, etc.) per mole of a substance. It is equal to 6.022 * 10^{23} mol-1 and is expressed as the symbol NA.

Hence, the relationship between number of moles and number of atoms is given as;

1 mole = 6.022 * 10^{23} atoms

The question asks to find the number of moles 3.25 * 10^{25} atoms equals to.

so we have;

1 = 6.022 * 10^{23}

x = 3.25 * 10^{25}

upon cross multiplication, we are left with;

x = (1 * 3.25 * 10^{25} ) / 6.022 * 10^{23}

x = 53.97 moles

charle [14.2K]3 years ago
3 0
Mole<span>: the amount of a substance that contains 6.02 x </span>10<span>. 23 respective particles of that substance. Avogadro's number: 6.02 x </span>10<span>. 23. Molar Mass: the mass of one </span>mole<span> of an element. CONVERSION FACTORS: 1 </span>mole<span> = 6.02 x </span>10<span>. 23 </span>atoms<span> 1 </span>mole<span> = </span>atomic<span> mass (g). Try: 1. How </span>many atoms<span> are in 6.5</span>moles<span> of zinc</span>
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An 80 kg long jumper in flight accelerates at a rate of 10 m/s^2. What is the force of the long jumper
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Answer:

F = 800 N

Explanation:

Given data:

Mass = 80 Kg

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Solution:

Formula:

<em>F = m × a </em>

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Now we will put the values in formula:

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3 years ago
a 125 g chunk of aluminum at 182 degrees Celsius was added to a bucket filled with 365 g of water at 22.0 degrees Celsius. Ignor
Diano4ka-milaya [45]
<h3>Answer:</h3>

32.98°C

<h3>Explanation:</h3>

We are given the following;

Mass of Aluminium as 125 g

Initial temperature of Aluminium as 182°C

Mass of water as 265 g

Initial temperature of water as 22°C

We are required to calculate the final temperature of the two compounds;

First, we need to know the specific heat capacity of each;

Specific heat capacity of Aluminium is 0.9 J/g°C

Specific heat capacity of water is 4.184 J/g°C

<h3>Step 1: Calculate the Quantity of heat gained by water.</h3>

Assuming the final temperature is X°C

we know, Q = mcΔT

Change in temperature, ΔT = (X-22)°C

therefore;

Q = 365 g × 4.184 J/g°C × (X-22)°C

    = (1527.16X-33,597.52) Joules

<h3>Step 2: Calculate the quantity of heat released by Aluminium </h3>

Using the final temperature, X°C

Change in temperature, ΔT = -(X°- 182°)C (negative because heat was lost)

Therefore;

Q = 125 g × 0.90 J/g°C × (182°-X°)C

  = (20,475- 112.5X) Joules

<h3>Step 3: Calculating the final temperature</h3>

We need to know that the heat released by aluminium is equal to heat absorbed by water.

Therefore;

(20,475- 112.5X) Joules = (1527.16X-33,597.52) Joules

Combining the like terms;

1639.66X = 54072.52

             X = 32.978°C

                = 32.98°C

Therefore, the final temperature of the two compounds will be 32.98°C

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