A quantity of steam (275g) at 110 degrees C is condensed and the resulting water is frozen into ice at 0 degrees C. How much heat was removed? Solve using kcal. Please solve by showing steps, I'm getting lost somewhere!
A mean calorie is 1?100 of the amount of energy required to warm one gram of air-free water from 0
1. Change temp from 110 to 100.
2. Convert steam into water.
3. Change temp from 100 to 0.
4. Convert water into ice.
1. 275 * .48 * 10 = 1320
2. 275 * 540 = 148500
3. 1 * 275 * 100 = 27500
4. 275 * 80 = 22000
1320 + 148500 + 27500 + 22000 = 199320 cal = 199.32 kcal
A quantity of steam (275g) at 110 degrees C is condensed and the resulting water is...
A quantity of steam (500 g) at 118°C is condensed, and the resulting water is frozen into ice at 0°C. How much heat was removed?
25 g steam at 110 ℃ is added temperature of the resulting water 100 g of ice at -10 ℃ in an insulated container. What is the final temperature of the resulting water?
25 g steam at 110 ℃ is added temperature of the resulting water 100 g of ice at -10 ℃ in an insulated container. What is the final temperature of the resulting water?
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
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...
MCQ7 (4 marks) Five statements are given below (i) f heat is supplied to ice at -10°C some ice always melts. (i) The heat evolved by steam at 110-C condensing to water at 100C is (mass) x (latent heat). (iii) If more heat than (mass) x (latent heat) is removed from ice at O'C the final temperature will be <oc (h) lf less heat than (mass) x (latent heat) is removed from ice at 0"C the final temperature will be>...
How much heat must be removed when 102 g of steam at 144°C is cooled and frozen into 102 g of ice at 0°C. (Take the specific heat of steam to be 2.01 kJ/kg·K.) I got 67 but its wrong.
.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...
BY TWO METHODS Steam at 150°C and I atm is to be condensed to 100°C and latm using cooling water in a continuous adiabatic heat exchanger. Cooling water enters at 20°C and leaves at 40°C. For each kg of steam condensed, calculate the mass (kg) of cooling water required using two different methods.
A Student wants to convert 75.0 g of ice at 0 degrees C to 75.0 g of liquid water at 60 degrees C. a) Sketch the heating curve on the axis for the melting of 75g of ice at 0 degrees C followed by the subsequent heating of the water formed to 60 degrees C. b) What is the total heat needed to melt the 75g of ice? c) What is the total amount of heat required to raise the...