Questions Q1. How many calories would be needed to vaporize 200.00 g water that you heated to its boiling point? Heat of vaporization for water is 540 cal/g. Show work Q2. What is the total amount of calories needed to 1) heat 200.00 g f water from 21.5 °C to its boiling point, and 2) to vaporize it? Show work

How much heat (in cal) is needed to heat a container of water (with a mass of 5 kg) (specific heat 1.00 cal/g deg C) from 34 deg Celsius to boiling (100 deg Celsius)?

a. The methanol in an automobile engine must be in the gas phase before it can react. Calculate the heat (in kJ) that must be added to 1.00 kg of liquid methanol in order to increase its temperature from 25.0°C to its normal boiling point of 65.0°C. The molar heat capacity of liquid methanol is 81.6 J/K*mol. b. Once the methanol has reached its boiling point, it must be vaporized. The molar enthalpy of vaporization, AHvap, for methanol is 38 kJ/mol. How much heat must be added to vaporize 1.00 kg of methanol?

A 52.03 g sample of a substance is initially at 28.5 °C. After absorbing 1165 J of heat, the temperature of the substance is 110.4 °C. What is the specific heat (?) of the substance? c=

Al is heated to 100 oC and dropped into a 100 gram glass beaker that contains 200 grams of H2 The temperature of the glass and water is 20 oC.  The final temperature of the system is 47 oC.  ( specific heat of Al = 0.29 J/gCo , specific heat of glass = 0.84 J/gCo )  What is the mass of aluminum that was used?

1. What is the specific heat of a 10. g sample of a substance that requires 950 J of heat to raise its temp from 18 °C to 42 °C? 2. Hg has a specific heat of 0.14 J/g°C. How much energy does a 22.8 g sample of mercury lose as its temp goes from 33 °C to 16 °C?

What is the amount of heat (value of q) when 22.8 g of gold is heated from 20.0℃ to 425℃? The specific heat capacity of gold is Cs,Au = 0.129 J/g℃. Select one: a. 2.94 J b. –1.19 x 10^3 J c. 405 J d. none of these e. –52.2 J f. 1.07 x 10^3 J g. 52.2 J h. 1.19 x 10^3 J i. –1.07 x 10^3 J j. –405 J

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 13.2 g, and its initial temperature is -12.7 °C. The water resulting from the melted ice reaches the temperature of his skin, 30.0 °C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.

* 00 A 0.535 g sample of steam at 103.9 °C is condensed into a container with 4.75 g of water at 15.3 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 the specific heat of steam is 2.01 , and AH van = 40.7 kJ/mol. g. "C g. C 9:19 AM 10/15/2021 TIL F2 F4 F5 F7 F8 F12 PrtScr Insert Delete 并 $ + Backspace 4. %3D 7. } { 1 K Enter H. M Shift C. B. Alt Ctrl Home PgDn

What change in energy is required to heat 55.00 g of water at 15.00 0C to vapor at 180.0 0C?