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4 years ago

A solution has [OH-] of 1x10^-2, what is the pOH of this solution

Chemistry

1 answer:

Brrunno [24]4 years ago

4 0

Answer:

The answer is: [D]: "12" .

Explanation:

i just did it

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What is the answer for this question

cestrela7 [59]

Answer:

The answer to your question is the second choice

Explanation:

Formula to calculate the heat of any substance

Q cal= mCcal ΔTcal

Formula to calculate the heat of a metal. The heat will be negative because it releases heat.

Qm = -mCmΔTm

Now equal both formula

Qcal = Q m

mCcalΔTm = -mCmetΔTmet

-Solve for Cmet

Cmet = -[mCcalΔTm] / mΔTmet

6 0

3 years ago

Which images show a container holding a heterogeneous mixture?

marshall27 [118]

Answer:

Explanation:

a heterogeneous mixture is one that is not uniform in composition.It is made up of non-uniform mix of smaller constituent parts that could be separated from one another using various means.

4 0

3 years ago

Read 2 more answers

Which of the following substances is less dense in its solid form than in its liquid form?

mojhsa [17]

Dude... h2o, thats why ICE FLOATS ON WATER!!!!

8 0

4 years ago

Read 2 more answers

Consider the balanced equation for the following reaction:

Zanzabum

<u>Answer:</u> The amount of carbon dioxide formed in the reaction is 5.663 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 oxygen gas = 8 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{8g}{32g/mol}=0.25mol$

For the given chemical equation:

$7O_2(g)+2C_2H_6(g)\rightarrow 4CO_2(g)+6H_2O(l)$

By Stoichiometry of the reaction:

7 moles of oxygen gas produces 4 moles of carbon dioxide

So, 0.25 moles of oxygen gas will produce = $\frac{4}{7}\times 0.25=0.143mol$ 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 = 0.143 moles

Putting values in equation 1, we get:

$0.143mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(0.143mol\times 44g/mol)=6.292g$

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 = 90 %

Theoretical yield of carbon dioxide = 6.292 g

Putting values in above equation, we get:

$90=\frac{\text{Experimental yield of carbon dioxide}}{6.292g}\times 100\\\\\text{Experimental yield of carbon dioxide}=\frac{90\times 6.292}{100}=5.663g$

Hence, the amount of carbon dioxide formed in the reaction is 5.663 grams

7 0

3 years ago

List two processes from which it may be concluded that the particles of a gas move continuously.

ziro4ka [17]

Answer:

The two processes maybe:

One process can be the spread of smell of perfume . Tge particles of perfume mic in the air and reaches every corner of tge room because they are moving

Second can be the smell of food that reaches us in seconds . This case too tells that the aroma of the food particles gets intermixed and come to us .

5 0

4 years ago