How much work is done on the steam when 1.32 mol of water at 100°C boils and becomes 1.32 mol of steam at 100°C at 1.00 atm pressure? (Assume the latent heat of vaporization of water is 2.26  106 J/kg.)

What is the value of the heat absorbed or emitted by liquid water of mass m = 410 g at 12° C to take it to the solid state at -15°C? Take Lf = 333 kJ/kg, the specific heat capacity of ice is 2220 J/kg • K, and the specific heat capacity of liquid water is 4186.8 J/kg • K.

In a mixing chamber, water at m ̇_1=1 kg/s flow rate, P1= 5 MPa and T1= 100 oC and water vapor at m ̇_2=5 kg/s flow rate, P2= 5 MPa and T2= 500 oC are mixed and Saturated steam is obtained at P3=5 MPa pressure. Calculate the amount of heat transfer (kW) lost from the mixing chamber to the environment at 20 oC.

A shipment from Earth to Mars contains a 50 gallon​ [gal] tank filled with an ideal gas. The molecular weight of the ideal gas is 15.9 grams per mole​ [g/mol]. NASA tells the astronauts on Mars that the tank and gas combined had an initial total mass of 5 kilograms​ [kg] and the pressure was 3 atmospheres​ [atm] before it left the Earth. During the​ trip, the temperature was kept constant at 20 degrees Celsius ​[°​C]. When it arrives on​ Mars, the astronauts check the sensors and discover the pressure is 2.2 atmospheres​ [atm] and the temperature is 20 degrees Celsius ​[°​C]. Based on this​ information, the astronauts determine that some of the gas leaked during shipment. Determine how much gas leaked from the tank in units of grams​ [g]. Gravity on Mars​ = 3.71 meters per second squared​[m/s2​].

A thirsty nurse cools a 2.40 L bottle of a soft drink (mostly water) by pouring it into a large aluminum mug of mass 0.249 kg and adding 0.122 kg of ice initially at -14.3 ∘C. If the soft drink and mug are initially at 21.0 ∘C, what is the final temperature of the system, assuming no heat losses? Express your answer in degrees Celsius.

An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, find the change in thermal energy and its final temperature.

If you have 6 moles of a diatomic ideal gas (such as oxygen or nitrogen), how much heat is required to raise the temperature of this gas from 261.5K to 282K if the volume of the gas remains constant during the heating?

A car engine burns 10 Ibm of fuel (equivalent to addition of QH) at 2600 R and rejects energy to the radiator and the exhaust at an average temperature of 1300 R. If the fuel provides 17 200 Btu/lbm what is the maximum amount of work the engine can provide?

A vertical cylinder with a heavy piston contains air at 300 K. The initial pressure is 2.00 × 105 Pa, and the initial volume is 0.350 m3. Take the molar mass of air as 28.9 g/mol and assume CV = 5/2 R. (a) Find the specific heat of air at constant volume in units of J/kg ? °C. (b) Calculate the mass of the airin the cylinder. (c) Suppose the piston is held fixed. Find the energy input required to raise the temperature of the air to 700 K. (d) What If? Assume again the conditions of the initial state and assume the heavy piston is free to move. Find the energy input required to raise the temperature to 700 K.

Water with a mass of mW = 0.400 kg and temperature of TW = 15.5°C is poured into an insulated bucket containing mI = 0.19 kg of ice at a temperature of TI = -15°C. Assume the specific heats of ice and water are constant at cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively. The latent heat of fusion for water is Lf = 334×103 J/kg.  Part (a)  What is the final temperature of the mixture, in degrees Celsius?  Tfinal =         Part (b)  Enter an expression for the mass of ice, in kilograms, that has melted when the mixture reaches its final temperature.  mmelt =     Part (c)  Calculate how much ice, in kilograms, has melted when the mixture reaches its final temperature.  mmelt =