#3 Question 1 : We have a bomb calorimeter with a heat capacity of 555 J/K. In this bomb calorimeter, we place 1000.0 mL of water. We burn 2.636 g of…


Question 1  : 

We have a bomb calorimeter with a heat capacity of 555 J/K. In this bomb calorimeter, we place 1000.0 mL of water. We burn 2.636 g of a solid in this bomb calorimeter. The temperature of the bomb calorimeter and the water increases by 2.29 oC. The molar mass of the solid is 593.8 g/mol. How much heat (in kJ) will be released if we were to burn 0.170 mol of this same solid in the bomb calorimeter? Keep in mind that we want to find the amout of heat released. The specific heat capacity or water is 4.184 J/K/g. Approximate the density of water as being exactly 1.00 g/mL. 

Question 2  : 

The standard enthalpies of formation, at 25.00 oC, of methane (CH4(g)), water (H2O(l)), and carbon dioxide (CO2(g)) are, respectively, -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the amount of heatreleased (in kJ) during the combustion of 18.89 L of methane under a constant pressure of 1.000 atm at 25.00 oC (N.B. combustion is the reaction with molecular oxygen to produce water and carbon dioxide.) 

Question 3  : 

We place a metal rod weighing 5.00 g with a specific heat capacity of 0.358 J/K/g in 24.0 mL of water. The specific heat capacity of water is 4.184 J/K/g and we make the approximation that its density is exactly 1.000 g/mL. The water has an initial temperature of 20.0 oC and the metal rod has an initial temperature of 80.8 oC. What is the final temperature (in oC) of the water and metal rod?

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