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प्रश्न
A child running a temperature of 101°F is given an antipyrin (i.e. a medicine that lowers fever) which causes an increase in the rate of evaporation of sweat from his body. If the fever is brought down to 98 °F in 20 min, what is the average rate of extra evaporation caused, by the drug? Assume the evaporation mechanism to be the only way by which heat is lost. The mass of the child is 30 kg. The specific heat of human body is approximately the same as that of water, and latent heat of evaporation of water at that temperature is about 580 cal g–1.
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उत्तर १
Initial temperature of the body of the child, T1 = 101°F
Final temperature of the body of the child, T2 = 98°F
Change in temperature, ΔT = `[(101 - 98 xx 5/9)]` °C
Time taken to reduce the temperature, t = 20 min
Mass of the child, m = 30 kg = 30 × 103 g
Specific heat of the human body = Specific heat of water = c
= 1000 cal/kg/ °C
Latent heat of evaporation of water, L = 580 cal g–1
The heat lost by the child is given as: `triangle theta = mc triangleT`
`= 30xx1000xx(101-98)xx5/9`
= 50000 cal
Let m1 be the mass of the water evaporated from the child’s body in 20 min.
Loss of heat through water is given by:
`triangle theta = m_1L`
`:. m_1 = (triangle theta)/L`
`= 50000/580 = 86.2 g`
∴Average rate of extra evaporation caused by the drug = `m_1/t`
`= 86.2/200 = 4.3 "g/min"`
उत्तर २
Decrease of temperature, Δt
`= 101^@ F - 98^@ F = 3^@ F = 3xx5/9 ""^@C = 1.67^@C`
Specific heat of water = `1000 "cal kg"^(-1) ""^@C^(-1)`
heat lost = `30 kg xx 1000 "cal kg"^(-1) ""^@C^(-1) xx 1.67 ""^@C = 50100 "cal"`
if m' be the mass of water evaporated then
`m' = (50100 " cal")/(580xx10^3xx "cak kg"^(-1)) = 0.086 kg`
This much water has taken 20 minutes to evaporate.
So rate of evaporation = `(0.086 kg)/(20 min) = (86 g)/(20 min)`
= 4.3 g`"min"^(-1)`
संबंधित प्रश्न
Given below are observations on molar specific heats at room temperature of some common gases.
| Gas |
Molar specific heat (Cv) (cal mol–1 K–1) |
| Hydrogen | 4.87 |
| Nitrogen | 4.97 |
| Oxygen | 5.02 |
| Nitric oxide | 4.99 |
| Carbon monoxide | 5.01 |
| Chlorine | 6.17 |
The measured molar specific heats of these gases are markedly different from those for monatomic gases. Typically, molar specific heat of a monatomic gas is 2.92 cal/mol K. Explain this difference. What can you infer from the somewhat larger (than the rest) value for chlorine?
What do you understand by the following statements:
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