Question
In: Chemistry
At 1 atm, how much energy is required to heat 55.0g of H2O(s) at -22.0 ^degree...
At 1 atm, how much energy is required to heat 55.0g of H2O(s) at -22.0 ^degree C to H2O(g) at 169.0^degree C?
Solutions
Expert Solution
q1 = mc
t
= 55*2.087*(0-(-22)
= 55*2.087*22 = 2525.27J
q2 = m * heat of fustion
= 55*333.6 = 18348J
q3 = mct
= 55*4.184*(100-0)
= 23012J
q4 = m*heat of vaporisation
= 55*2257
= 124135J
q5 = mct
= 55*2*(169-100)
= 55*2*69
= 7590J
q = q1+ q2+q3+q4+q5
= 2525.27+18248+23012+124135+7590 =
175510J = 175.51KJ
queen_honey_blossom answered 2 years agoRelated Solutions
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6010. J/mol Enthalpy of vaporization 2257 J/g
40660 J/mol Specific heat of solid H2O (ice)
2.087 J/(g·°C) *
37.60 J/(mol·°C) * Specific heat of liquid
H2O (water)
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