Answers:
Calculations are given in image
14. q= 4.975 kcal
15. delT= 66.086 oC
16. m = 28.8 g
18. p = 0.75 atm
22. V= 0.270 L
Question 14 of 39 > How much heat is required to raise the temperature of 26.2...
< Question 7 of 19 > The temperature of a sample of aluminum increased by (23.3- \text{°C}\) when (269\text{J}W) of heat was applied What is the mass of the sample? Substance lead silver Specific heat J/g. °C) 0.128 0.235 0.385 0.449 0.903 copper iron aluminum Vm=10) W\text{g} \0
(a) How much heat is required to raise by 15.70°C the temperature of 1.1 kg of water. (b) How much heat is required to raise by 15.70°C the temperature of 1.1 kg of iron.
(a) How much heat is required to raise by 12.40°C the temperature of 1.8 kg of water. (b) How much heat is required to raise by 12.40°C the temperature of 1.8 kg of iron.
How much heat is required to raise by 11.70°C the temperature of 1.2 kg of iron.
R55150 < Question 21 of 22 > The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 3.17 g of water boils at atmospheric pressure? heat: about us Careers privacy policy terms of use contact us help
heat in terms of kcals not kJ How much heat is required to raise the temperature of 11.1 g of water from -45°C to 175 °C? heat: kcal
How much heat energy is required to convert 45.2 g of a solid iron at 28 C to liquid iron at 1538 C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 C. The specific heat capacity of solid iron is 0.449 J/ (g • C). Question 6 of 6 > How much heat energy is required to convert 45.2 g of solid iron at 28 °C to liquid iron at...
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
8. How much heat is needed to raise the temperature of 100 copper pennies weighing 3.012 g each from 25.2°C to 40.7°C (assuming the pennies are ca. 100% Cu, and the specific heat of Cu=0.385J/g.°C).
How much heat (in kJ) is required to raise the temperature of 288.7 g of ethanol (mw=46.07) from 39.38 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)