A 100 g sample of an unknown liquid absorbs 2000 J of heat energy, raising the liquid’s temperature from 50 ◦ C to 70 ◦ C . What is the speciﬁc heat capacity of this liquid? No phase change took place.
When 1 kg of ice at 0 degrees Celsius absorbs 80 kilocalories of heat, the ice undergoes a) a change of state b) a loss of energy c) a rise in temperature d) an increase in volulme The heat of fusion of water is 80 kcal/kg. That
1.) A vapor volume of 1.17 L forms when a sample of liquid CH3CN absorbs 1.00 KJ of heat at its normal boiling point (81.1 C and 1 atm). What is the heat of vaporization in KJ per moles of CH3CN? 2.) The vapor pressure of water at
Some heat is supplied to a mixture of ice and liquid water in a closed container and the contents of the container are thoroughly mixed. If, after the addition of heat, both ice and liquid water remain: A) the temperature of the
When ice at 0°C melts to liquid water at 0°C, it absorbs 0.334 kJ of heat per gram. Suppose the heat needed to melt 30.7 g of ice is absorbed from the water contained in a glass. If this water has a mass of 0.189 kg and a
When a block of ice at zero degrees Celcius melts, the ice absorbs energy from its environment. As the ice is melting, the temperature of the block (remains the same, increase decrease) I think it remains the same. A sample of
Can you please help me figure out why evaporation is a cooling process and why becoming a solid is a heating process? evaporation absorbs heat from the environment, thus "cooling" the environment. becoming solid is a heating