A mass m of steam at 130º C is used to warm 200 gm of water from 20º C to 50º C.  Write an expression in terms of mass, m, for the heat lost by the steam as it cools to its boiling point.  Write an expression in terms of mass, m, for the heat lost as the water condenses from the steam and then cools to the final equilibrium temperature of 50º C. Then calculate the amount of heat gained by the water, Q gained, raising its temperature from 20º C to 50º C and find the initial mass of the steam needed to complete this process as described.

The velocity versus time graph for an object is shown in the diagram below. (b) v (t) B to C C to D D to E (a) What is the direction of the acceleration of the object for each of the indicated time intervals? A to B negative direction ✓ positive direction the acceleration is zero positive direction. --Select-- positive direction B negative direction the net force is zero D V What is the direction of the net force acting on the object for each of the indicated time intervals? A to B ---Select--- B to C C to D D to E E, t (s)

A kettle brings 2.15 kg of water at 34.9˚C to steam at 110˚C.  How much heat does this take?    The specific heat of water is 4186 J/kg˚C, The specific heat of ice is 2090 J/kg˚C, and the specific heat of steam is 2010 J/kg˚C  The latent heat of fusion for water is 3.33 x 105 J/kg and the latent heat of vaporization for water is 2.26 x 106 J/kg

In an experiment measuring the latent heat of fusion of water, the following procedure was followed. Ice cube of mass 35.0 g at an initial temperature of 0.0°C is dropped into 225.0 g of 65.0°C water in an aluminum container. The mass of the aluminum container is 44 .0 g and the final equilibrium temperature is 46.0℃. Determine whether any heat is lost or gained in this experiment to the environment. If yes, how much? (For water: c = 1.00 cal/g×°C and Lf = 77.9 cal/g; for Al: c = 0.215 cal/g×°C

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 16.8 g, and its initial temperature is -10.7 °C. The water resulting from the melted ice reaches the temperature of his skin, 29.4 '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.

A CANDU nuclear reactor produces steam at 350 deg C to drive a steam-electric turbine.  the temperature of the condensed steam when it returns to the boiler is 30.0 deg C.  Calculate the heat extracted from each 100 kg of the steam?Please give a step by step and include givens. Thanks!!

A certain mass, m, of water has thermal energy added to it until the water is at the boiling point.  Additional thermal energy is added until the entire mass, m, has been phased changed into steam.   a) The temperature of the steam will be less than that of the water at the boiling point.  b) The temperature of the steam will be greater than that of the water at the boiling    point.  c) The temperature of the steam will be the same as that of the water at the boiling    point.  d) The temperature of the steam will be zero.  e) The temperature of the steam will be 2256000K.

The initial temperature of 60 g of ice is -200C. The specific heat capacity of ice is 0.5 cal/g.C0 and water’s is 1 cal/g.C0. The latent heat of fusion of water is 80 cal/g. How much heat is required to raise the ice to 00C and completely melt the ice? (b) How much additional heat is required to heat the water (obtained by melting the ice) to 620C?

A chocolate bar has 225Cal. Charlie is locked in a deserted chocolate factory and needs to heat 2.00L of water for his dinner. He plans on burning chocolate bars to accomplish this. a) How many kJ of energy are needed to heat the water from 25.0C to 100.0C? __ kJ b) What fraction of a chocolate bar would be needed to heat the water?  __% Answer all parts A and B.

When you turn your hot water on in the shower, it takes a bit for the water to get warm. Some of this is because the water in the pipe is cold but some of it is because the water from the hot water heater must heat the copper plumbing pipe itself. Copper has a specific heat of 0.39R. How much energy does it take to heat 2 kilograms of copper pipe from 70°F to 130°F? Report your answer in Joules. (Hint: Note that you'll need to convert kJ to J and F to K.)