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Neporo4naja [7]
3 years ago
10

60 х 8 у x= 04 09 O 16

Chemistry
1 answer:
vovikov84 [41]3 years ago
7 0

Answer:

The answer is 16

Explanation:

It needs to be hald of the medium so devide the 2 numbers

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What is the boiling point of a solution of 76 g of water dissolved in 500 mL of acetic acid, CH3COOH?
tatuchka [14]

Answer:

127.3° C, (This is not a choice)

Explanation:

This is about the colligative property of boiling point.

ΔT = Kb . m . i

Where:

ΔT = T° boling of solution - T° boiling of pure solvent

Kb = Boiling constant

m = molal (mol/kg)

i = Van't Hoff factor (number of particles dissolved in solution)

Water is not a ionic compound, but we assume that i = 2

H₂O →  H⁺  +  OH⁻

T° boling of solution - 118.1°C =  0.52°C . m . 2

Mass of solvent =  Solvent volume / Solvent density

Mass of solvent = 500 mL / 1.049g/mL → 476.6 g

Mol of water are mass / molar mass

76 g / 18g/m = 4.22 moles

These moles are in 476.6 g

Mol / kg = molal → 4.22 m / 0.4766 kg = 8.85 m

T° boling of solution =  0.52°C . 8.85 m . 2 + 118.1°C =  127.3°C

6 0
3 years ago
Read 2 more answers
Mercury is a liquid meteal but it is not hard? how can we say it is a metal
NNADVOKAT [17]
What's the problem ? Hardness is not the definition of a metal. You need to expand your thinking. EVERY element is solid, liquid, and gas, over different ranges of temperature ... including all of the metals. There are only TWO elements that are liquid AT ROOM TEMPERATURE, and mercury is one of them. But on a mild day at the south pole, mercury is solid too.
7 0
3 years ago
The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: E = R_y/n^2 In this equation R_y stands
Katarina [22]

Answer:

The wavelength of the line in the emission line spectrum of hydrogen caused by the transition of the electron for the given energy levels is 5.23\times 10^{-5} m

Explanation:

Given :

The energy E of the electron in a hydrogen atom can be calculated from the Bohr formula:

E=\frac{R_y}{n^2}

R_y=2.18\times 10^{-18} J =  Rydberg energy

n =  principal quantum number of the orbital

Energy of 11th orbit = E_{11}

E_{11}=\frac{2.18\times 10^{-18} J}{11^2}=1.80\times 10^{-20} J

Energy of 10th orbit = E_{10}

E_{10}=\frac{2.18\times 10^{-18} J}{10^2}=2.18\times 10^{-20} J

Energy difference between both the levels will corresponds to the energy of the wavelength of the line which can be calculated by using Planck's equation.

E'=E_{10}-E_{11}=2.18\times 10^{-20} J-1.80\times 10^{-20} J

=E'=0.38\times 10^{-20} J

\lambda =\frac{hc}{E'} (Planck's' equation)

\lambda = \frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{0.38\times 10^{-20} J}

\lambda = 5.2310\times 10^{-5} m\approx 5.23\times 10^{-5} m

The wavelength of the line in the emission line spectrum of hydrogen caused by the transition of the electron for the given energy levels is 5.23\times 10^{-5} m

3 0
3 years ago
Zinc metal reacts with copper sulfate through the following
morpeh [17]

Answer:

26.9

Explanation:

5 0
2 years ago
How many moles of oxygen are needed to burn 425g of sulfur
Anika [276]
I believe 212.5m, but I may be wrong, I’m a little rusty with moles
3 0
3 years ago
Read 2 more answers
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