How much heat is gained by copper when21.8 g of copper is warmed from 15.5 degree...
How much heat is gained by nickel when 29.2 g of nickel is warmed from 18.3°C to 69.6°C? The specific heat of nickel is 0.443 J/(g. °C). 0 2.37 × 10², 09.00 x 102, 22.73 6.64 x 102) 30.8) Question 11 (1 point) A 170.0-g sample of metal at 78.0°C is added to 170.0 g of H2O() at 15.0°C in an insulated container. The temperature rises to 17.9°C. Neglecting the heat capacity of the container, what is the specific heat...
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree C to gaseous ethanol at 167.4 degree C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 degree C and a normal boiling point of 78.4 degree C. The specific heat capacity of liquid ethanol is 2.45 J/g middot degree C and that of gaseous ethanol...
How much heat do you need if you want to raise the temperature of 31.0g of copper from 10.0 degree celsius to 60.0 degree celsius? (The specific heat of copper is 0.385 J/g degree celsius).
How much heat must be added to a 8.0-kg Nock of ice at -8 degree C to change it to water at 14 degree C? The specific heat of ice is 2050)/kg middot C degree. the specific heat of water is 4186 J/kg middot C degree, the latent heat of fusion of ice is 334,000 J/kg. and 1 cal = 4.186 J. A) 140 kcal B) 780 kcal C)730kcal D)810kcal E) 180 kcal
36. How much heat is gained by nickel when 500 g of nickel is warmed from 22.4 to 584"C? me specific 0.444 J/KB C). 37. Given the following data of the standard enthalpy changes, find the heat required for the reaction converting solid sulfur to gaseous sulfur at 298 K and I atm pressure. heat of nickel is A) 2000J B 4000 C) 60003D) 8000 E) 100003 A)-1013k/rnol B)+618klmol C)-618 kimiol D)-223 kinol E)+223 kinnol 38. Calculate the standard heat...
How much heat must be removed from 456 g of water at 25.0 degree C to change it into ice at -10.0 degree C? The specific heat of ice is 2090 J/kg K. the latent heat of fusion of water is 33.5 times 10^4 J/Kg, and the specific heat of water is 4186 J/kg K.
The specific heat of a certain type of cooking oil is 1.75 J/(g middot degree C). How much heat energy is needed to raise the temperature of 2.48 kg of this oil from 23 degree C to 191 degree C?
You pour 210 g hot coffee at 78.7 degree C and some cold cream at 7.50 degree C to a 115-g cup that is initially at a temperature of 22.0 degree C. The cup, coffee, and cream reach an equilibrium temperature of 63.0 degree C. The material of the cup has a specific heat of 0.2604 kcal/(kg middot degree C) and the specific heat of both the coffee and cream is 1.00 kcal/(kg middot C). If no heat is lost...
If 400 J of heat were added to 100 g copper (specific heat = 0.385 J/g°C) and 400 J were added to 100 g of gold (specific heat = 0.129 J/g°C), which metal, copper or gold, would have the lower final temperature?
Copper metal has a specific heat of 0.385 J/g·°C. Calculate the amount of heat required to raise the temperature of 22.8 g of Cu from 20.0°C to 875°C. a. 1.0 × 10-2 J b. 1.97 × 10-5 J c. 7.51 kJ d. 329 J e. 10.5 kJ