Calculate the energy change (with the correct sign) when the temperature of 100.0 mL of liquid...

Calculate the energy change (with the correct sign) when the temperature of 100.0 mL of liquid water increases by 4.40 °C.

Calculate the mass of NaO2CCH3 needed to release this amount of energy when dissolved in water. ΔHsolution(NaO2CCH3) = -989.5 J/mol.

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Expert Solution

specific heat capacity of water, C = 4.186 J/goC
density of water = 1 g/mL
Volume = 100 mL
Mass of water = density * volume = 1 * 100 = 100 g

Q = m*C*(Tf-Ti)
     = 100*4.186*(4.4)
    =1842 J
Answer: 1842 J
-----------------------------------------
delta H solution = -989.5 J/mol
number of moles of NaO2CCH3 required = 1842 J / 989.5 J/mol = 1.86 mol
Molar mass of NaO2CCH3 =23 + 2*16 + 2*12 + 3*1= 82 g/mol
mass of NaO2CCH3 = number of moles * molar mass
                                        = 1.86 mol * 82 g/mol
                                        = 152.5 g
Answer: 152.5 g

queen_honey_blossom answered 1 year ago

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