At 1 atm, how much energy is required to heat 71.0 g of H2O(s) at –22.0 °C to H2O(g) at 169.0 °C?
q = m * s * dT + dH fusion * n + m * s* dT + dH vapourisation *n
q = 71 * 2.05 *(0+22) + 6.02 * (71/18) + 71 * 4.184 * (100-0) + 71* 2.02 * (169-100) + 40.17*(71/18)
q = 42986.67 J
q = 42.99 kJ
At 1 atm, how much energy is required to heat 71.0 g of H2O(s) at –22.0...
At 1 atm, how much energy is required to heat 71.0 g of H2O(s) at − 20.0 °C to H2O(g) at 171.0 °C? Heat transfer constants can be found in this table.
At 1 atm, how much energy is required to heat 51.0 g of H2O(s) at –22.0 °C to H2O(g) at 141.0 °C?
At 1 atm, how much energy is required to heat 75.0 g H2O(s) at −22.0 ∘C to H2O(g) at 147.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 55.0g of H2O(s) at -22.0 ^degree C to H2O(g) at 123.0^degree C? Please answer in kJ & explain in detail
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At 1 atm how much energy is required to heat 85.0 (g) of H2O (s) at -22.0 degrees celsius to H2O (g) at 141.0 degrees celsius?
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