$$ \qquad $$ (1) $$ Q_{1 C F}=c \mathrm{mDt}=2.03 \mathrm{~J} / \mathrm{g} \cdot \mathrm{C} \cdot 95 \mathrm{~g} \cdot 12^{\circ} \mathrm{C}=2,314.2 \mathrm{~J}=2.3142 \mathrm{~kJ} $$ (2) $$ \Delta H_{f}=\frac{95 \mathrm{~g} H_{1} \mathrm{O}\left|\operatorname{lmol}_{18 \mathrm{D}}\right| 6.02 \mathrm{~kJ}}{18.02 \mathrm{~g} H_{50} \mid \mathrm{lmolH}_{2} \mathrm{D}}=31.7 \mathrm{~kJ}=31.7 \mathrm{~kJ} $$ (3) $$ Q_{\text {wattr }}=c m \Delta t=4.18 \mathrm{~J} / \mathrm{g} \cdot \mathrm{C} \cdot 95 \mathrm{~g} \cdot 25^{\circ} \mathrm{C}=9,927.5 \mathrm{~J}=9.92 \mathrm{~J} \mathrm{~kJ} $$ $$ +43.9 \mathrm{~kJ} $$ Rewatch Released (D) Mull 2) Is this energy released or absorbed? Absorbed Released

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UpStudy AI · Accepted Answer

1. Calculation (1):  
   The energy calculated is  
   $$
   Q_{1CF} = c \, m \, \Delta t = 2.03 \, \frac{\text{J}}{\text{g} \cdot \text{°C}} \times 95 \, \text{g} \times 12\, \text{°C} = 2314.2 \, \text{J} = 2.3142 \, \text{kJ}
   $$

2. Calculation (2):  
   The enthalpy change of formation is  
   $$
   \Delta H_{f} = \frac{95\, \text{g}\, H_2O \times 6.02\, \frac{\text{kJ}}{\text{lmol}}}{18.02\, \text{g}\, H_2O} = 31.7 \, \text{kJ}
   $$

3. Calculation (3):  
   The energy change for water is calculated as  
   $$
   Q_{\text{water}} = c \, m \, \Delta t = 4.18\, \frac{\text{J}}{\text{g} \cdot \text{°C}} \times 95 \, \text{g} \times 25\, \text{°C} = 9927.5 \, \text{J} = 9.9275 \, \text{kJ} \approx 9.92 \, \text{kJ}
   $$

4. Total energy change:  
   The total energy change is given as  
   $$
   +43.9 \, \text{kJ}
   $$  
   Since the energy change is positive, this indicates that the system has absorbed energy.

5. Answer to the question:  
   The energy is absorbed.
The calculations show that the system absorbed a total of 43.9 kJ of energy.

(1)
(2)
(3)

Rewatch
Released
(D) Mull
2) Is this energy released or absorbed?
Absorbed
Released

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(1) (2) (3) Rewatch Released (D) Mull 2) Is this energy released or absorbed? Absorbed Released