2.4l= 2400mldensity= 1ml/gMass= 1× 2400= 2400g= 2.4kgWater boils at 0°CBoiling point = 100°CInitial = 20°CSpecific heat capacity of water = 4200j/kg/°C= 4200×(100-20)×2.4= 806400j= 806.400kJ
1 Answers 1 viewsHeat needed =7,208.78cal
1 Answers 1 viewsEnthalpy of vaporization for water is 2260 kJ/kg. Thus, the amount of RELEASED heat will be Q = r*m = 2260 kJ/kg*0.010 kg = 22.6 kJ or 5.4 kcal.
1 Answers 1 viewsq = 4520 kJ = 4520000 J.Solution:For water at its normal boiling point of 100 ºC, the heat of vaporization (Hv) is 2260 J g-1. This means that to convert 1...
1 Answers 1 viewsThe density of water is 0.998 g/mL. Therefore the mass = 100 x 0.998 = 99.8 g.q = cm(T2 - T1) = 1.00cal/goC x 99.8g x 20oC = 1996 calAnswer:...
1 Answers 1 views80 calories needed to melt 1gm ICE at 0 degree.Hence for 90 gm ICE, it require 80x90 = 7200 calories So answer = 7200 calories.
1 Answers 1 viewsQUESTION # 132550Calculate the heat needed at 0∘C∘to make each of the following changes of state.Calories to melt 22 g of iceANSWERSΔHf = q/mWhere;ΔHf = enthalpy of fusion of water(80cal/gram)q...
1 Answers 1 viewsSolutions: Meters (m) and centimeters (cm) can be related by the prefix modifier equality 100 cm = 1 m.So therefore, this equality given above can be represented as two conversion...
1 Answers 1 viewsSpecific latent heat of vaporization of water at 100°C = 2260 J/gHeat change = (13.0 g) × (2260 J/g) = 29380 J = 7022 cal;Answer: 7022 calories
1 Answers 1 views5.2°C = (273 + 5.2)k = 278.2kChange in temperature = 368k -278.2= 89.8kq (heat energy) = MCp∆TWhen Cp of water =1046J q = 7.59 g × 1046J × 89.8k =...
1 Answers 1 views