Burns produced by steam at 100°C are much more severe than those produced by the same mass of 100°C water. To verify this:
(a) Calculate the heat that must be removed from 4.00 g of 100°C
water to lower its temperature to 48.0°C.
kcal
(b) Calculate the heat that must be removed from 4.00 g of 100°C
steam to condense it and lower its temperature to 48.0°C.
kcal
(c) Calculate the mass of human flesh that the heat produced in
each case can raise from the normal 37.0°C to 48.0°C. (Flesh is
badly damaged at 50.0°C.)
steam
kg
water
kg
Burns produced by steam at 100°C are much more severe than those produced by the same...
Burns produced by steam at 100 degree C are much more severe than those produced by the same mass of 100 degree C water. To verify this, answer the questions below. Specific heat of water = 1.00 kcal/(kg degree C); heat of vaporization = 539 kcal/kg; specific heat of human flesh = 0.83 kcal/(kg degree C). Calculate the quantity of heat that must be removed from 7.00 g of 100degree C water to lower its temperature to 45.0degree C. kcal...
Burns produced by steam at 100°C are much more severe than those produced by the same mass of 100°C water. To verify this: (a) Calculate the heat that must be removed from 6.00 g of 100°C water to lower its temperature to 53.0°C. ________kcal (b) Calculate the heat that must be removed from 6.00 g of 100°C steam to condense it and lower its temperature to 53.0°C. ________kcal (c) Calculate the mass of human flesh that the heat produced in...
Calculate the energy released when 50.0g of steam condenses at 100℃.Use the cooling curve to show what happens when 50.0g steam condenses at 100℃ and then cools to 20℃. Then calculate this energy change.6. Use the below cooling curve for water for the following questions. A. Label the melting/freezing point. B. Label the boiling/evaporation point. C. At what state is water when the temperature is 80 °c? D. At what state is water when the temperature is -20 °C? E. What happens to the temperature...
Steam at 100°C is condensed into a 54.0 g copper calorimeter cup containing 300 g of water at 21.0°C. Determine the amount of steam (in g) needed for the system to reach a final temperature of 48.0°C. The specific heat of copper is 387 J/(kg · °C).
.1. A 2.50 kg block of ice at 0°C is added to a picnic cooler. How much heat (in kcal) will the ice remove as it melts to water at 0°C? 2. A 300.0 g pot of water at room temperature (25.0°C) is placed on a stove. How much heat (in kcal) is required to change this water to steam at 100.0°C? 3. Spent steam from an electric generating plant leaves the turbines at 110.0°C and is cooled to 95.0°C liquid water...
A 50.0-g copper calorimeter contains 260 g of water at 20.0°C. How much steam at 100°C must be condensed into the water if the final temperature of the system is to reach 45.0°C? g
iPad 6:32 PM * 33% Exit A 50.0 g silver spoon at 20.0°C is placed in a cup of coffee at 90.0°C. How much heat (in kcal) does the spoon absorb from the coffee to reach a temperature of 89.0°C? (Assume Csilver-0.056 kcal/kgC.) Question 13 1 pts A 200.0 g china serving bowl is warmed 65.0°C when it absorbs 2.6 kcal of heat from a serving of hot food. What is the specific heat of the china dish? Question 14...
Calculate the final equilibrium temperature when 10.0 grams of steam initially at 100 degree C is mixed with 450 grams of liquid water and 110 grams of ice at 0 degree C in a calorimeter. That is, the liquid water AND the ice are initially at 0 degree C. Ignore any heat energy exchanges with the calorimeter and the surroundings. If you conclude that the final temperature of the system is 0 degree C, then what mass of ice remains,...
the amount of steam (in g) needed for the system to reach Steam at 100°C is condensed into a 54.0 g steel calorimeter cup containing 300 g of water at 23.0°C a final temperature of 64.0°C. The specific heat of steel is 490 3/(kg °C).
Calculate how many grams of ice at 0°C would be melted by 100 g of 100°C steam. Hint: heat will be transferred from the steam to the ice in two processes: •the steam will condense into liquid, and •that liquid will transfer heat until it is at the freezing point of water. Note that for water: Lf = 80 cal/g (ice), and Lv = 540 cal/g (steam) (Use calories) C(water) =1 cal/g*C Answer in grams no decimal places.