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Nostrana [21]
1 year ago
14

What is the change in internal energy (in J) of a system that absorbs 0.615 kJ of heat from its surroundings and has 0.247 kcal

of work done on it?
Chemistry
1 answer:
Radda [10]1 year ago
7 0

The change in internal energy of a system is 1648.45 J.

First we convert calories into joule :-

From question, values are given q = 0.615 kJ

                                                     q  = 615 J

                                                  w = 0.247 kcal

                                                  w = 247 Cal = 247 × 4.184 J

                                                  w = 1033.45 J

Formula of change in internal energy, ΔE = q + w

Here, the system absorbs heat from surroundings, so q is positive

Now, put the values of q and w in the formula,

ΔE = q + w

ΔE = 615 + 1033.45 J

ΔE = 1648.45 J

Internal energy is the sum of ability power of the gadget and the machine's kinetic strength. The alternate in internal energy (ΔU) of a response is equal to the heat gained or lost (enthalpy trade) in a reaction whilst the reaction is administered at steady pressure. Inside the study of thermodynamics, a usually perfect gasoline is taken into consideration as a running substance. The molecules of an ideal gasoline are mere mass points that exert no force on each other.

The SI derived unit used to degree strength or paintings. One joule is identical to the electricity used to accelerate a body with a mass of 1 kilogram using one newton of force over a distance of one meter. One joule is also equal to one watt-second.

Learn more about internal energy here:- brainly.com/question/1370118

#SPJ4

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Answer:

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strojnjashka [21]
<span>Determine the root-mean-square sped of CO2 molecules that have an average Kinetic Energy of 4.21x10^-21 J per molecule. Write your answer to 3 sig figs.
</span><span>
E = 1/2 m v^2 

If you substitute into this formula, you will get out the root-mean-square speed. 

If energy is Joules, the mass should be in kg, and the speed will be in m/s. 

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If you divide this by Avagadro's constant, you will get the average mass of a CO2 molecule. 

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A 32.5 g iron rod, initially at 22.4 ∘C, is submerged into an unknown mass of water at 63.0 ∘C, in an insulated container. The f
Allisa [31]

Answer:

The mass of water m_{w} = 39.18 gm

Explanation:

Mass of iron m_{iron} = 32.5 gm

Initial temperature of iron T_{1} = 22.4°c = 295.4 K

Specific heat of iron  C_{iron} = 0.448 \frac{KJ}{kg K}

Mass of water = m_{w}

Specific heat of water  C_{w} = 4.2 \frac{KJ}{kg  K}

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Final temperature after equilibrium T_{f} = 59.7°c = 332.7 K

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Heat lost by water  = Heat gain by iron rod

m_{w} C_{w} (T_{2} - T_{f} ) =  m_{iron} C_{iron} ( T_{f} - T_{1} )

Put all the values in above formula we get

m_{w} × 4.2 × ( 336 - 332.7 ) = 32.5 × 0.448 × ( 332.7 - 295.4 )

m_{w} = 39.18 gm

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