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Marrrta [24]
2 years ago
11

How many molecules of N2O5 are there in 175 grams of N2O5?

Chemistry
1 answer:
Vaselesa [24]2 years ago
6 0

Answer:

9.76 x 10²³molecules

Explanation:

Given parameters:

Mass of N₂O₅  = 175gram

Unknown:

Number of molecules  = ?

Solution:

To find the number of molecules contained in the given mass, we need to find the number of moles of N₂O₅ first.

   Number of moles  = \frac{mass}{molar mass}

 Molar mass of N₂O₅ = 2(14) + 5(16) = 108g/mol

  Number of moles = \frac{175}{108}   = 1.62moles

  Now;

               1 mole of a substance  = 6.02 x 10²³ molecules

              1.62 mole of N₂O₅  = 1.62 x 6.02 x 10²³  = 9.76 x 10²³molecules

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3 years ago
Elements chemically combine in various ways to form most substances on Earth. These chemically combined elements are called ____
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Answer:

compounds

Explanation:

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Read 2 more answers
A solution is prepared by dissolving 42.0 g of glycerin, C3H8O3, in 186 g of water with a final volume of 200.0 mL. a. Calculate
trapecia [35]

<u>Answer:</u>

<u>For a:</u> The molality and molarity of the given solution is 2.45m and 2.28 M respectively.

<u>For b:</u> The molarity of the solution when more water is added is 0.912 M

<u>Explanation:</u>

  • <u>For a:</u>

To calculate the molality of solution, we use the equation:

Molarity=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}

Where,

m_{solute} = Given mass of solute (C_3H_8O_3) = 42.0 g

M_{solute} = Molar mass of solute (C_3H_8O_3) = 92.093 g/mol

W_{solvent} = Mass of solvent (water) = 186 g

Putting values in above equation, we get:

\text{Molality of }C_3H_8O_3=\frac{42\times 1000}{92.093\times 186}\\\\\text{Molality of }C_3H_8O_3=2.45m

  • To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}    .....(1)

We are given:

Molarity of solution = ?

Molar mass of (C_3H_8O_3) = 92.093 g/mol

Volume of solution = 200 mL

Mass of (C_3H_8O_3) = 42 g

Putting values in above equation, we get:

\text{Molality of }C_3H_8O_3=\frac{42\times 1000}{92.093\times 200}\\\\\text{Molality of }C_3H_8O_3=2.28M

Hence, the molality and molarity of the given solution is 2.45m and 2.28 M respectively.

  • <u>For b:</u>

Now, the 300 mL water is added to the solution. So, the total volume of the solution becomes (200 + 300) = 500 mL

Using equation 1 to calculate the molarity of solution, we get:

Molar mass of (C_3H_8O_3) = 92.093 g/mol

Volume of solution = 500 mL

Mass of (C_3H_8O_3) = 42 g

Putting values in equation 1, we get:

\text{Molality of }C_3H_8O_3=\frac{42\times 1000}{92.093\times 500}\\\\\text{Molality of }C_3H_8O_3=0.912M

Hence, the molarity of the solution when more water is added is 0.912 M

5 0
3 years ago
What is likely to be found in placer deposit
Dmitriy789 [7]
In geology, a placer deposit<span> or </span>placer<span> is an accumulation of valuable minerals formed by gravity separation during sedimentary processes. ... Valuable mineral components often occurring with black sands are monazite, rutile, zircon, chromite, wolframite, and cassiterite.</span>
8 0
3 years ago
A liquid is exposed to infrared radiation with a wavelength of 6.92 × 10 − 4 cm. 6.92×10−4 cm. Assume that all the radiation is
Anastaziya [24]

Answer:

The no. of photons required for total heat absorbed of 58.28 J is N = 20.28  × 10^{22} Photons

Explanation:

Wave length \lambda = 6.92 × 10^{-4} cm =  6.92 × 10^{-6} m

Total Energy E = 58.28 J

Energy content of a single photon is given by

E = \frac{hc}{\lambda}

where h = plank constant = 6.626 × 10^{-34} J - s

c = speed of the light = 3 × 10^{8} \frac{m}{s}

So Energy content of a single photon is

E = \frac{(6.626) (3)}{6.92} × 10^{-22}

E = 2.87 × 10^{-22} J

No. of photons required is

N = \frac{Total\ energy}{energy \ of \ a \ single \ photon}

N = \frac{58.28}{2.87} × 10^{22}

N = 20.28  × 10^{22} Photons

This is the no. of photons required for total heat absorbed of 58.28 J

5 0
2 years ago
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