Solve Question 4 only 3. An experiment was conducted in which 100. mL of water w

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Solve Question 4 only
3. An experiment was conducted in which 100. mL of water was reacted with 15.6001 g of nitrate. The heat capacity of the calorimeter was 132 J/C. Use this information and to answer the following questions. Assume that the specific heat of the solution equals Table 1 that of water. Table 1. Heat of Solution (rc) Temperature of room Temperature of 100 mL H0 Temperature of ammonium nitrate Lowest temperature after mixing 25.0 25.0 25.0 15.0 A. Calculate the heat released by water (5 pts). B. Calculate the heat released by the calorimeter (5 pts). 1- 132 / X (5-15)1326 T C. Calculate the heat of the reaction (5 pts). - Determine the identity of an unknown diatomic gas with a density of 3.16 g/L at STP (10 pts). (Hint: Determine the molar mass.] 4. 25

Explanation / Answer

3. As the temperature of the mixture after reaction is lower than before, we can say that the reaction is endothermic. Heat of reaction is provided by the sensible heat from cooling of the mixture and the calorimeter.

A. Assuming constant density of water 1 g/ml

Heat released by water=> 100 mL * 1g/ml * 4.184 J/°C g * (25°C-15°C)

=> 4184 J => 4.184 kJ

B. Heat released by calorimeter=> heat capacity * T

=> 132 J/°C * (25°C - 15° C)

=> 1320 J => 1.32 kJ

C. Then heat of reaction=> heat from calorimeter + heat from water

=> 4.184 kJ + 1.32 kJ=> 5.50 kJ

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