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notsponge [240]
3 years ago
5

What is ΔE in kJ for a system that receives 1.79 kJ of heat from surroundings and has 4.51 kcal of work done on it at the same t

ime. 1 cal = 4.184 J.
Chemistry
1 answer:
kenny6666 [7]3 years ago
4 0

Answer: 20.7 kJ

Explanation:

According to first law of thermodynamics:

\Delta E=q+w

\Delta E=Change in internal energy

q = heat absorbed or released

w = work done or by the system

w = work done on the system=-P\Delta V  {Work is done on the system is positive as the final volume is lesser than initial volume}

w = 4.51 kcal = 4.51\times 4.184kJ=18.9kJ    (1kcal = 4.184kJ)

q = +1.79 kJ   {Heat absorbed by the system is positive}

\Delta E=+1.79+(18.9)=20.7kJ

Thus \Delta E for a system that receives 1.79 kJ of heat from surroundings and has 4.51 kcal of work done on it at the same time is 20.7 kJ

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Answer:

  • <em><u>3</u></em>

Explanation:

Please, find the  image with the pictured molecule for this question attached.

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<em>Hydrogen bondings</em> are intermolecular bonds (bonds between atoms of two different molecules not between atoms of the same molecule). The hydrogen bonds are attractions between the positive end of one hydrogen atom and the negative end of a small atom of other molecule (N, O, or F).

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A soft drink that contains 47 grams of carbohydrates per serving has a nutritional calories (cal) per serving of 188 calories.

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In order to get the number of nutritional calories per serving from a soft drink that has 47 grams of carbohydrate, we will need to multiply the number of grams by 4 since there are about 4 calories for every gram of carbohydrate, and the calculation is as follows:

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