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3 years ago

What is the wavelength of infrared radiation with a frequency of 3.85 x 10^12 Hz?

Chemistry

1 answer:

ELEN [110]3 years ago

3 0

Answer:

Wavelenght is 7,79x10⁻⁵ m

Explanation:

The equation that connects wavelentgh (λ) and frequency (ν) is:

λ=c/ν

Where c is speed of light (3x10⁸ m/sec) and λ is expressed in lenght´s units and ν is expressed in "time⁻¹ " units (for example, sec⁻¹)

According to the details, if we just replace the given value of frequency, we just obtaing wavelenght data:

λ= (3x10⁸ m/sec)/(3,85x10¹² sec⁻¹) = 7,79x10⁻⁵ m

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jalyn ran at speed of 3 m/s then came to a sudden stop during a time period of 3 s. what was his acceleration

tensa zangetsu [6.8K]

Answer:

I believe the answer is 1m/s²

Explanation:

acceleration= change in speed ÷ time (I hope this is correct)

4 0

3 years ago

X2o3 express you answer as a whole number

kobusy [5.1K]

<span>2.40 - 1.68 =0.72 g of oxigen
moles = 0.72/16 g/mol=0.045

moles x = 1.68/ 55.9=0.03

0.03/0.03 = 1 = x
0.045 / 0.03 = 1.5 = O

to get whole numbers multiply by 2

x2O3

X2O3 +3 CO = 2 X + 3 CO2</span>

4 0

3 years ago

How many atoms are there in 8.88 g Si?

Mariana [72]

Answer:

$\boxed {\boxed {\sf 1.90 \times 10^{23} \ atoms \ Si}}$

Explanation:

We are asked to find how many atoms are in 8.88 grams of silicon.

<h3>1. Grams to Moles </h3>

First, we convert grams to moles. We use the molar mass or the mass of 1 mole of a substance. These values are found on the Periodic Table as they are equal to the atomic masses, but the units are grams per mole instead of atomic mass units.

Look up silicon's molar mass.

Si: 28.085 g/mol

We will convert using dimensional analysis. Set up a conversion factor with the molar mass.

$\frac { 28.085 \ g \ Si}{1 \ mol \ Si}$

We are converting 8.88 grams of silicon to moles, so we multiply by this value.

$8.88 \ g \ Si *\frac { 28.085 \ g \ Si}{1 \ mol \ Si}$

Flip the fraction so the units of grams of silicon cancel.

$8.88 \ g \ Si *\frac{1 \ mol \ Si} { 28.085 \ g \ Si}$

$8.88 *\frac{1 \ mol \ Si} { 28.085 }$

$\frac {8.88} { 28.085 } \ mol \ Si$

$0.316183015845 \ mol \ Si$

<h3>2. Moles to Atoms </h3>

Next, we convert moles to atoms. We use Avogadro's Number or 6.022 × 10²³. This is the number of particles (atoms, molecules, formula units, etc.) in 1 mole of a substance. In this case, the particles are atoms of silicon.

Set up another conversion factor.

$\frac {6.022 \times 10^{23} \ atoms \ Si}{1 \ mol \ Si}$

Multiply by the number of moles we calculated.

$0.316183015845\ mol \ Si *\frac {6.022 \times 10^{23} \ atoms \ Si}{1 \ mol \ Si}$

The units of moles of silicon cancel.

$0.316183015845 * \frac {6.022 \times 10^{23} \ atoms \ Si}{1}$

$0.316183015845 * {{6.022 \times 10^{23} \ atoms \ Si}$

$1.90405412 \times 10^{23} \ atoms \ Si$

<h3>3. Significant Figures</h3>

The original measurement of 8.88 grams has 3 significant figures, so our answer must have the same.

For the number we calculated, that is the hundredth place. The 4 in the thousandth place tells us to leave the 0 in the hundredth place.

$1.90 \times 10^{23} \ atoms \ Si$

<u>8.88 grams of silicon contains 1.90 ×10²³ atoms of silicon.</u>

6 0

3 years ago

Given the following list of densities, which materials would float in a molten vat of lead provided that they do not themselves

vampirchik [111]

Answer:

b. glass and charcoal

Explanation:

Step 1: Given data

Density of Pb: 11.4 g/mL

Density of Glass: 2.6 g/mL

Density of Au: 19.3 g/mL

Density of charcoal: 0.57 g/mL

Density of platinum: 21.4 g/mL

Step 2: Determine which material will float in molten lead

Density is an intrinsic property of matter. Less dense materials float in more dense materials. The materials whose density is lower than that of lead and will therefore float on it are glass and charcoal.

8 0

3 years ago

How many grams of S are in 475 g of SO2?

enot [183]

There are 237. 5 g of Sulfur,S in 475 g of SO2?

<h3 />

<h3>Calculation of grams of Sulfur</h3>

From the question, we can say that

The molar mass of sulfur = 32 g/mol

The molar mass of oxygen = 16 g/mol

Therefore,

The molar mass for SO2 = 32 + (16 × 2) g/mol = 64 g/mol

Now,

If 1 mole of SO2 contains 1 mole of S

Then 64 g of SO2, will contain 32g of S;

Such that

475 g of SO2 will give { $\frac{ 32g of S) ( 475 g of SO2)}{64 of SO2}$ } = 237. 5 g of Sulfur.

Learn more about molar mass here :brainly.com/question/18291695

6 0

2 years ago