Question
The change in enthalpy for NaOH dissolved in water is . When a 19.9 g sample is dissolved in 500.0 g of water in a coffee-cup calorimeter, what is the final temperature of the system? Presume the specific heat of the solution is the same as that of liquid water.
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Answer to a math question The change in enthalpy for NaOH dissolved in water is . When a 19.9 g sample is dissolved in 500.0 g of water in a coffee-cup calorimeter, what is the final temperature of the system? Presume the specific heat of the solution is the same as that of liquid water.
Esmeralda
4.795 Answers
1. Convert the mass of NaOH to moles: \frac{19.9 \, \text{g}}{40.0 \, \text{g/mol}} = 0.4975 \, \text{mol}
2. Calculate the heat released:0.4975 \, \text{mol} \times -44.51 \, \text{kJ/mol} = -22.14 \, \text{kJ}
3. Convert kJ to J:-22.14 \, \text{kJ} \times 1000 \, \text{J/kJ} = -22140 \, \text{J}
4. Calculate the temperature change:
\Delta T = \frac{-22140 \, \text{J}}{519.9 \, \text{g} \times 4.18 \, \text{J/g}^\circ \text{C}} = -10.23 \, ^\circ \text{C}
5. Determine the final temperature:
25 \, ^\circ \text{C} + (-10.23 \, ^\circ \text{C}) = 14.77 \, ^\circ \text{C}
[Answer] \( 14.77 \, ^\circ \text{C} \)
2. Calculate the heat released:
3. Convert kJ to J:
4. Calculate the temperature change:
5. Determine the final temperature:
[Answer] \( 14.77 \, ^\circ \text{C} \)
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