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How much heat is needed to bring 12.0 g of water from 28.3 °C to 43.87 °C, if the specific heat capacity of water is 4.184 J/(g•°C)?

Sagot :

Lanuel

Answer:

Heat capacity, Q = 781.74 Joules

Explanation:

Given the following data;

Mass = 12g

Initial temperature = 28.3°C

Final temperature = 43.87°C

Specific heat capacity of water = 4.184J/g°C

To find the quantity of heat needed?

Heat capacity is given by the formula;

[tex] Q = mcdt [/tex]

Where;

Q represents the heat capacity or quantity of heat.

m represents the mass of an object.

c represents the specific heat capacity of water.

dt represents the change in temperature.

dt = T2 - T1

dt = 43.87 - 28.3

dt = 15.57°C

Substituting into the equation, we have;

[tex] Q = 12*4.184*15.57 [/tex]

Q = 781.74 Joules

The heat that should be needed is Q = 781.74 Joules.

  • The calculation is as follows;

Heat capacity should be

= mcdt

Where;

Q represents the heat capacity or quantity of heat.

m represents the mass of an object.  

c represents the specific heat capacity of water.  

dt represents the change in temperature.

Now

dt = T2 - T1

= 43.87 - 28.3

= 15.57°C

Now

[tex]= 12\times 4.184 \times 15.57[/tex]

= 781.74 joules

Learn more: brainly.com/question/16911495