How much heat does it take to increase the temperature of 1.45 L of water from 0 deg Celsius to 100 deg Celsius? Assume water has a density of 1 g/mL
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Expert's answer
2017-03-22T09:49:56-0400
Solution: Specific heat capacity is given by formula S=(q÷(m×∆T))S=(q÷(m×∆T)), Where: s = specific heat capacity (sometimes represented by the letter c, or Cs) q = heat m = mass (we can calculate mass of water, using equation: m = ρ∙V = 1g/mL∙1450mL = 1450 (g)) Δ T = change in temperature: ∆T = 100 - 0 = 100. As per Specific Heat Capacity of Water, 4.184 J of heat is required to raise temperature of 1 g of water by 1 ℃. So, the value of heat is: q = S∙m∙∆T = 4.184∙1450∙100 = 606680 (J) = 606.68 (kJ)
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