I don't understand this problem<br>?Mg+?02=?Mg0

What is the energy of a photon with a frequency of 3.2 x 10 -2 Hz?

Anestetic [448]

Answer:

E = 21.22 ×10⁻³⁶ J

Explanation:

Given data:

Energy of photon = ?

Frequency of photon = 3.2×10⁻² Hz

Solution:

Formula:

E = hf

h = 6.63×10⁻³⁴ Js

Now we will put the values in formula.

E = 6.63×10⁻³⁴ Js × 3.2×10⁻² Hz

E = 21.22 ×10⁻³⁶ J (Hz= s⁻¹)

5 0

3 years ago

What causes the expression of a recessive trait? one dominant and one recessive factor (allele) one dominant gene two recessive

murzikaleks [220]

Answer: i think it’s two recessive alleles

Explanation:

6 0

3 years ago

When [H+] = 3.33 x 10-7 what is the ph?

Fittoniya [83]

Answer:

Explanation:

The pH of a solution can be found by using the formula

$pH = - log ([ {H}^{+} ])$

From the question we have

$pH = - log(3.33 \times {10}^{ - 7} ) \\ = 6.477555...$

We have the final answer as

Hope this helps you

8 0

3 years ago

Dissolving potassium chlorate (KClO3) is even more endothermic than potassium chloride.

zhenek [66]

Answer:

The mass of KClO₃ that will absorb the same heat as 5 g of KCl is 3.424 g

Explanation:

Here we have

Heat of solution of KClO₃ = + 41.38 kJ/mol.

Heat of solution of KCl (+17.24 kJ/mol)

Therefore, 1 mole of KCl absorbs +17.24 kJ during dissolution

Molar mass of KCl = 74.5513 g/mol

Molar mass of KClO₃ = 122.55 g/mol

74.5513 g of KCl absorbs +17.24 kJ during dissolution, therefore, 5 g will absorb

$\frac{17.24}{74.5513 } \times 5 \, \, kJ \, or \, 1.156 \, kJ$

Therefore the amount of KClO₃ to be dissolved to absorb 1.156 kJ of energy is given by

122.55 g of KClO₃ absorbs + 41.38 kJ, therefore,

$\frac{1.156}{41.38} \times 122.55 \, g = 3.424 \, g$

Therefore the mass of KClO₃ that will absorb the same heat as 5 g of KCl = 3.424 g.

5 0

3 years ago

. A compound contains only C, H, N, and O. It contains 37.0 % C and 42.5% O (both by mass), and there are 2 O atoms for every 1

jasenka [17]

Answer:

C₂₁H₁₅N₉O₁₈

Explanation:

Molecular formula is the ratio of atoms that are present in 1 molecule of the compound. We need to find moles of all atoms to find this ratio.

In a basis of 100, moles of C and O are:

<em>Moles C:</em>

37.0 * (1mol / 12g) = 3.083 moles C

<em>Moles O: </em>

42.5g * (1mol / 16) = 2.656 moles O

Now, to find moles of H, we need determine moles of H2O produced:

0.0310g H2O * (1mol / 18g) = 1.72x10⁻³ moles H2O * 2 = 3.44x10⁻³ moles H

These moles were produced when 0.157g of the compound react. In a basis of 100g:

3.44x10⁻³ moles H * (100g / 0.157g) = 2.194 moles H

In the same way, moles of N are:

0.0230g NH3 * (1mol / 17g) = 1.35x10⁻³ moles H2O

These moles were produced when 0.103g of the compound react. In a basis of 100g:

1.35x10⁻³ moles H * (100g / 0.103g) = 1.313 moles N

Empirical formula is (The simplest whole number ratio of atoms presents in a molecule). Dividing in the low number of moles (Moles N):

C: 3.083 moles C / 1.313 moles N = 2.3

O: 2.656 moles O / 1.313 moles N = 2.0

N: 1.313 moles N / 1.313 moles N = 1

H: 2.194 moles H / 1.313 moles N = 1.67

This ratio times 3 (To have the whole number ratio):

C: 7

O: 6

N: 3

H: 5

The empirical formula is:

C₇H₅N₃O₆

And weighs:

C: 7*(12g/mol)= 84

H: 5 * (1g/mol) = 5

N: 3 * (14g/mol) = 42

O: 6* (16g/mol) = 96

227g/mol

As the molecular mass of the compound is 681g/mol:

681 / 227 = 3

The empirical formula times 3 is the molecular formula, that is:

C₇H₅N₃O₆ × 3

4 0

3 years ago

I don't understand this problem?Mg+?02=?Mg0​

I don't understand this problem?Mg+?02=?Mg0