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dsp73
4 years ago
12

Use the dropdown to create a unbalanced diagram with the dog using Applied Force pulling to the right.

Chemistry
1 answer:
Ber [7]4 years ago
7 0
Is there an image with this question
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How many joules of energy are required to melt 125 g of water?
marissa [1.9K]

Answer for this question is 45,000

3 0
3 years ago
While in Europe, if you drive 119 km per day, how much money would you spend on gas in one week if gas costs 1.10 euros per lite
Mkey [24]
We have to convert:
1 km = 0.62173 mi
1 lit = 0.264172 gallons
119 * 0.62173 = 73.943 mi per day
73.943 : 30 = 2.4648 gal per day
2.4648 : 0.264172 * 1.10 = 10.26 Euros per day
<em>In one week :
</em>10.26 * 7 = 71.28 Euros
71.28 * 1.26 = $90.50
Answer:   
You would spend $90.50 in one week.
4 0
4 years ago
Which of the following terms refers to the area immediately around the eye
Anit [1.1K]

Answer:

the eye socket

Explanation:

the area around the eye is called the eye socket or the eye orbit.

5 0
3 years ago
Which of the following is true about semipermanent membranes?
Leto [7]

Answer: It interferes with the movements of the fatty acid tails of the phospholipids

I hope this helps

4 0
4 years ago
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g)ΔH = −184.6 kJ / mol If 2.00 moles of H2 re
serious [3.7K]

Answer : The value of \Delta E of the reaction is, -369.2 KJ

Explanation :

Formula used :

\Delta E=\Delta H-\Delta n_g\times RT

where,

\Delta E = internal energy of the reaction = ?

\Delta H = enthalpy of the reaction = -184.6 KJ/mole = -184600 J/mole

The balanced chemical reaction is,

H_2(g)+Cl_2(g)\rightarrow 2HCl(g)

when the moles of H_2\text{ and }Cl_2 are 2 moles then the reaction will be,

2H_2(g)+2Cl_2(g)\rightarrow 4HCl(g)

From the given balanced chemical reaction we conclude that,

\Delta n_g = change in the moles of the reaction = Moles of product - Moles of reactant = 4 - 4 = 0 mole

R = gas constant = 8.314 J/mole.K

T = temperature = 25^oC=273+25=298K

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

\Delta E=(-184600J/mole\times 2mole)-(0mole\times 8.314J/mole.K\times 298K)

\Delta E=-369200J

\Delta E=-369.2KJ

Therefore, the value of \Delta E of the reaction is, -369.2 KJ

6 0
3 years ago
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