Physics, asked by bitsianrk9302, 1 year ago

Find the amount of heat supplied to decrease the volume of an ice water mixture

Answers

Answered by Jasleen0599
0

To decrease the volume of an ice water mixture we have to convert ice into water because ice is more dense than water that why ice float on water.

1. Q= mL . This is the amount of heat required to convert ice into water . Here L is latent heat of fusion.

Answered by bestwriters
0

Complete question:

Find the amount of heat supplied to decrease the volume of an ice water mixture by 1 \bold{cm^3} without any change in temperature.

\bold{(\rho_{ice}=0.9\rho_{water}; \ L_{ice}=80 \ cal/gm)}

A. 360 cal

B. 500 cal

C. 720 cal

D. None of these

Answer:

The amount of heat supplied to decrease the volume of an ice water mixture is 720 cal.

Given:

Volume = \bold{1 \ cm^3}

\bold{\rho_{ice}=0.9\rho_{water}}

\bold{L_{ice}=80 \ cal/gm}

To find:

Amount of heat supplied = ?

Formula:

\bold{Q=mL}

Where,

m = Mass

L = Enthalpy of fusion

Solution:

When the volume is decreased by \bold{1 \ cm^3} then the volume is \bold{9 \ cm^3}

Volume is converted to mass:

\bold{Mass=m =Density\times Volume =1000 \times 9\times 10^{-6}}

\bold{\therefore m = 9\times10^{-3} \ kg=9 \ gm}

Now, the amount of heat applied is:

\bold{Q=9\times 80}

\bold{\therefore Q = 720 \ cal}

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