Enthalpy and Hess's LawChemistry Lab Manual 2nd Edition3) When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, thereaction shown below occurs and the temperature of the resulting solution rises from 22.00Cto 33.10°C. If the specific heat of the solution is 4.18 J/(g. °C) , calculate AH for the reaction, aswritten.Ba(s) + 2 H2O()AH ?Ba(OH)2(aq) + H2(g)
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Enthalpy and Hess's Law Chemistry Lab Manual 2nd Edition 3) When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00C to 33.10°C. If the specific heat of the solution is 4.18 J/(g. °C) , calculate AH for the reaction, as written. Ba(s) + 2 H2O() AH ? Ba(OH)2(aq) + H2(g)
Given information:
Mass of barium = 1.50 g
Mass of water = 100.00 g
Initial temperature = 22.00 ◦C
Final temperature = 33.10 ◦C
Specific heat of the solution = 4.18 J/g. ◦C
Enthalpy of solution can be determined by measuring the amount of heat (q) released and number of moles of solute (n). The expression for enthalpy can be expressed as follows:
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ΔΗ-
The amount of heat released can ...
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q=m.C.AT =(1.50+100.00) gx4.18 J/g°Cx(33.10-22.00) °C =4709.397 J =4.709 kJ
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