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3 years ago

Hcl and 1-isopropylcyclohexane formation

Chemistry

2 answers:

Vanyuwa [196]3 years ago

8 0

Answer:

Spahgetti

Explanation:

Grace [21]3 years ago

3 0

Yes I don’t know what this means

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If Oxygen gains 2 electrons what charge will it have?

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A very powerful one

Explanation:

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3 years ago

What happens to water molecules when they are heated?

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Temperature causes water molecules to move more quickly, because each individual molecule has more energy as it gets hotter .

So, the answer is A.

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An electrically neutral atom of oxygen has eight electrons. What other facts do you know for sure about this atom? 1.) there are

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2.) there are eight protons

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3 years ago

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11. Assuming that the gases are ideal, calculate the amount of work done (joules) in each of the following reactions at 25 degre

gayaneshka [121]

Answer:

For a: Work done for the given reaction is 2477.572 J.

For b: Work done for the given reaction is 0 J

Explanation:

To calculate the work done for the reaction, we use the equation:

$W=-P\Delta V$

Ideal gas equation follows:

$PV=nRT$

Relating both the above equations, we get:

$W=-\Delta n_gRT$ ......(1)

where,

$\Delta n_g$ = difference in number of moles of products and reactants = $n_g_{(products)}-n_g_{(reactants)}$

R = Gas constant = 8.314 J/K.mol

T = temperature = $25^oC=[273+25]K=298K$

For a:

The chemical reaction follows:

$4HCl(g)+O_2(g)\rightarrow 2Cl_2(g)+2H_2O(g)$

$\Delta n_g=4-5=-1$

Putting values in equation 1, we get:

$W=-(-1mol)\times (8.314J/K.mol)\times 298K=2477.572J$

Hence, work done for the given reaction is 2477.572 J.

For b:

The chemical reaction follows:

$2NO(g)\rightarrow N_2(g)+O_2(g)$

$\Delta n_g=2-2=0$

Putting values in equation 1, we get:

$W=-(0mol)\times (8.314J/K.mol)\times 298K=0J$

Hence, work done for the given reaction is 0 J.

3 0

3 years ago

I NEED HELP :)

BlackZzzverrR [31]

Answer:

48 mph

Explanation:

total time= 19/12 hr

distence- 76 miles

speed- D/T=76/19/12

which is 48mph

if my answer helps please mark as brainliest.

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3 years ago

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