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4 years ago

If this is a p1000 micropipette, then this is set to dispense [ Select]ul. If this is a p10

Chemistry

1 answer:

mariarad [96]4 years ago

3 0

Answer:

1000 µL; 10 µL

Explanation:

A p1000 micropipet is set to dispense 1000 µL.

A p10 micropipet set to dispense 10 µL.

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I need help on either question you can answer. Thank you god bless

Stels [109]

<h3>Further explanation</h3>

1.Atomic Number (Z) = Mass Number (A) - Number of Neutrons

neutrons = mass number-atomic number

Atomic mass Cl-37= 17

Mass number Cl-37=37

Neutrons = 37-17=20

2. Mass atom X = mass isotope 1 . % + mass isotope 2.%...

$\tt atomic~mass~X=0.0224\times 88+0.7832\times 90+0.1944\times 91=90.1$

3. The energy in one photon can be formulated as

$\large{\boxed{\bold{E\:=\:h\:.\:f}}}$

f = c / λ, so :

$\tt E\approx f\approx \dfrac{1}{\lambda}$

Energy is directly proportional to frequency and inversely proportional to the wavelength

So, as the frequency of photon increases, the energy of photon increases

4. Based on answer number 3 :

A. The wavelength becomes longer, and the energy decreases

7 0

3 years ago

For the following reaction, 5.61 grams of carbon monoxide are mixed with excess water . Assume that the percent yield of carbon

stealth61 [152]

<u>Answer:</u> The ideal yield of carbon dioxide is 7.506 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of carbon monoxide = 5.61 g

Molar mass of carbon monoxide = 28 g/mol

Putting values in equation 1, we get:

$\text{Moles of carbon monoxide}=\frac{5.61g}{28g/mol}=0.200mol$

The chemical equation for the reaction of carbon monoxide and water follows:

$CO(g)+H_2O(l)\rightarrow CO_2(g)+H_2(g)$

By Stoichiometry of the reaction:

1 mole of carbon monoxide produces 1 mole of carbon dioxide

So, 0.200 moles of carbon monoxide will produce = $\frac{1}{1}\times 0.200=0.200mol$ of carbon dioxide

Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 0.200 moles

Putting values in equation 1, we get:

$0.200mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.200mol\times 44g/mol)=8.8g$

To calculate the experimental yield of carbon dioxide, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Percentage yield of carbon dioxide = 85.3 %

Theoretical yield of carbon dioxide = 8.8 g

Putting values in above equation, we get:

$85.3=\frac{\text{Experimental yield of carbon dioxide}}{8.8g}\times 100\\\\\text{Experimental yield of carbon dioxide}=\frac{85.3\times 8.8}{100}=7.506g$

Hence, the ideal yield of carbon dioxide is 7.506 grams

3 0

3 years ago

Using de Broglie's equation, λ = h/mv which would have a larger wavelength, a slow-moving proton or a fast-moving golf ball? Exp

TiliK225 [7]

Answer : The correct option is a slow-moving proton.

Explanation :

The de Broglie's equation is,

$\lambda =\frac{h}{mv}$

where,

$\lambda$ = wavelength of particle

h = Planck's constant

m = Mass of particle

v = speed of particle

From the de Broglie's equation, we conclude that there is an inverse relationship between the wavelength and speed or mass of particle. That means the lower the speed and mass of particle, higher will be the wavelength of particle and vice-versa.

So, a slow-moving proton have a larger wavelength due to slow speed of proton.

5 0

3 years ago

Four students give their teacher identical apples. Each student sets his or her apple on a different stack of books. Which

ycow [4]

D
explanation ; i’m smart

7 0

4 years ago

SOMEONE HELP ME PLEASE

Korolek [52]

Answer:

evaporation

Explanation:pls mark brainliest

6 0

2 years ago