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loris [4]
2 years ago
7

The frequency of an x-ray wave is 3.0 x 1012 MHz. Its wave speed is 3.0x 108 m/s. Calculate the wavelength of the x-ray wave bel

ow.
Can some one help!!
Chemistry
1 answer:
elena55 [62]2 years ago
6 0

Answer:

λ = 1*10⁻¹⁰m

Explanation:

Frequency (f) = 3.0*10¹²MHz = 3.0*10¹⁸Hz

Speed (v) = 3.0*10⁸m/s

Speed (v) of a wave = frequency (f) * wavelength (λ)

V = fλ

Solve for λ,

λ = v / f

λ = 3.0*10⁸ / 3.0*10¹⁸

λ = 1*10⁻¹⁰m

λ = 0.

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A pound is approximately 0.45 kilogram. A person weighs 87 kilograms. What is the person’s weight, in pounds, when expressed to
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4. Magnesium and oxygen undergo a chemical reaction to
erastovalidia [21]

Answer:

About 16.1 grams of oxygen gas.

Explanation:

The reaction between magnesium and oxygen can be described by the equation:
\displaystyle 2\text{Mg} + \text{O$_2$} \longrightarrow 2\text{MgO}

24.4 grams of Mg reacted with O₂ to produce 40.5 grams of MgO. We want to determine the mass of O₂ in the chemical change.

Compute using stoichiometry. From the equation, we know that two moles of MgO is produced from every one mole of O₂. Therefore, we can:

  1. Convert grams of MgO to moles of MgO.
  2. Moles of MgO to moles of O₂
  3. And moles of O₂ to grams of O₂.

The molecular weights of MgO and O₂ are 40.31 g/mol and 32.00 g/mol, respectively.

Dimensional analysis:

\displaystyle 40.5\text{ g MgO} \cdot \frac{1\text{ mol MgO}}{40.31\text{ g MgO}} \cdot \frac{1\text{ mol O$_2$}}{2\text{ mol MgO}} \cdot \frac{32.00\text{ g O$_2$}}{1\text{ mol O$_2$}} = 16.1\text{ g O$_2$}

In conclusion, about 16.1 grams of oxygen gas was reacted.

You will obtain the same result if you compute with the 24.4 grams of Mg instead:

\displaystyle 24.4\text{ g Mg}\cdot \frac{1\text{ mol Mg}}{24.31\text{ g Mg}} \cdot \frac{1\text{ mol O$_2$}}{1\text{ mol Mg}} \cdot \frac{32.00\text{ g O$_2$}}{1\text{ mol O$_2$}} = 16.1\text{ g O$_2$}

3 0
2 years ago
What is the total number of molecules in 11.2 liters of N2 gas at STP
scoray [572]
Molar volume at STP = 22,4 L

1 mole -------------- 22,4 L
 x mole -------------- 11,2 L

x = 11,2 / 22,4

x =  0,5 moles of N2

1 mole --------------- 6,02.10²³ molecules
0,5 moles ------------ y molecules

y = 0,5 . 6,02.10²³

y = 3,01.10²³ molecules 

7 0
3 years ago
How many grams of carbon is needed to react with hydrogen gas to produce 59.8 grams of acetylene (C2H2)?
Bad White [126]

Answer:

55.1657 grams/mol of carbon is needed to react with hydrogen gas to produce 59.8 grams of acetylene (C2H2)

Explanation:

The molecular weight of acetylene is  26.04 g/mol

Molecular weight of carbon is equal to 12.011 g/mol

Two carbon atom produces one acetylene molecule.

Thus, 2 * 12.011 g/mol of carbon is used to produce  26.04 g/mol of acetylene,

Amount of carbon required to produce 59.8 grams of acetylene

\frac{2*12.011}{26.04} * 59.8 \\= 55.1657grams/mol

55.1657 grams/mol of carbon is needed to react with hydrogen gas to produce 59.8 grams of acetylene (C2H2)

5 0
2 years ago
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