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3 years ago

PLEASE HELP ME I’ll give brainliest

Chemistry

1 answer:

sineoko [7]3 years ago

6 0

divide 5 hours 20 mins by 4,000

and ur answer is

320 mins/4000km

0.08

hope this helps

sorry if its wrong

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What is a feature shared by all animal cells?

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Answer:

1. Animal cells are eukaryotic

2. All live things are made up of cells (I think)

3. Cells are the basic unit of all living things

Explanation:

Number 2 is probably wrong because I can't see the diagram but, all living things ARE actually made up of cells

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3 years ago

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Scott is making a chart to show the difference between chemical reactions and nuclear reactions. Which part of his chart is inco

yanalaym [24]

Answer:

Line 3 is incorrect

Explanation:

In line 3, the statements should be switched. Chemical reactions involve small amounts of energy and nuclear reactions involve enourmous amounts of energy. Lines 1 and 2 are correct.

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The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 8.600 g C6H6 is burned and the heat pr

jenyasd209 [6]

Answer : The final temperature of the water is, $22.5166^oC$

Explanation : Given,

Mass of benzene = 8.600 g

Molar mass of benzene = 78 g/mole

First we have to calculate the moles of benzene.

$\text{Moles of benzene}=\frac{\text{Mass of benzene}}{\text{Molar mass of benzene}}=\frac{8.600g}{78g/mol}=0.1103mole$

Now we have to calculate the energy of combustion.

The given balanced chemical reaction is:

$2C_6H_6(l)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(l)+6542 kJ$

According to reaction,

As, 2 moles of benzene gives 6542 kJ of energy on combustion.

So, 0.1103 mole of benzene gives $\frac{6542 kJ}{2}\times 0.1103=360.7913kJ$ of energy on combustion.

Now we have to calculate the final temperature of the water.

Formula used : $q_w=m_w\times c_w\times \Delta T=m_w\times c_w\times (T_{final}-T_{initial})$

where,

$q_w$ = heat released = 360.7913 kJ = 36079.13 J

$m_w$ = mass of water = 5691 g

$c_w$ = specific heat of water= $4.18J/g^oC$

$T_{final}$ = final temperature = ?

$T_{initial}$ = initial temperature = $21^oC$

Now put all the given values in the above formula, we get:

$36079.13J=5691g\times 4.18J/g^oC\times (T_{final}-21^oC)$

$T_{final}=22.5166^oC$

Therefore, the final temperature of the water is, $22.5166^oC$

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