How many grams of ice (at 0.00 °C) would be melted by the energy obtained as 15.2 g of steam is condensed at 100°C and cooled to 22.1°C? ____g      Specific heat (ice) = 2.10 J/g°C      Specific heat (water) = 4.18 J/g°C      Heat of fusion = 333 J/g      Heat of vaporization = 2258 J/g NOTE: Answer must be in 3 significant figures.

Use the following values to answer each part. The specifi c heat of water is 1.00 cal/(g · °C); the heat of fusion of water is 79.7 cal/g; and the heat of vaporization of water is 540 cal/g. a. How much energy (in calories) is needed to melt 45 g of ice at 0.0 °C and warm it to 55 °C? b. How much energy (in calories) is released when 45 g of water at 55 °C is cooled to 0.0 °C, and frozen to solid ice at 0.0 °C? c. How much energy (in kilocalories) is released when 35 g of steam at 100. °C is condensed to water, the water is cooled to 0.0 °C, and the water is frozen to solid ice at 0.0 °C?

Some physical properties of water are shown below. melting point boiling point specific heat solid 2.05 J/g °C specfic heat liquid 4.184 J/g.°C specific heat gas 2.02 J/g °C ΔΗ° fusion 6.02 kJ/mol ΔΗ° vaporization 40.7 kJ/mol If 16.6 g of water at 80°C are mixed with 10.7 g of ice at 0.0°C, what is the final temperature of the mixture? °℃ 0.0°C 100.0°C

How much energy is needed to convert 59.5 grams of ice at 0.00 celsius to water at 60.9 celsius? specific heat(ice) = 2.10 J/g specific heat (water) 4.18 J/g heat of fusion= 6.02 kJ/mol heat of vaporization= 40.6 kJ/mol

20.) You want to raise the temperature of ice at 0 degrees Celsius to steam at 110 degrees O Celsius. The specific heat of water is 4.184 J/Cg. The specific heat of steam is 2.01 J/Cg, and the specific heat of ice is 2.03 J/Cg. Ice has a heat of fusion at 334 J/g and water has a heat of vaporization of 2260 J/g. Find the Q for this raise in temperature.

Ethanol (C2 H5 OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? 3949 207.3 6.67 8.97 -12.5

4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C? 5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to steam at 105.0 °C. How much heat would be released in the reverse process?

Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C