When 0.250 g of iron (atomic weight = 55.85 g/mol) is burned, 0.341 g of iron...

 

 

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When 0.250 g of iron (atomic weight = 55.85 g/mol) is burned, 0.341 g of iron oxide is obtained. What is the mass percent of iron in the iron oxide? Given that the atomic weight of Oxygen = 16.00 g/mol. %3D O a. 83.1% O b. 77.9% O c. 75.5% d. 73.3% e. 80.4% In a calorimeter calibration experiment, a sample of 55.50 g of water at 55.00 °C is added to a calorimeter containing 50.50 g of water at 20.00 °C After stirring and waiting for the system to equilibrate, the final temperature reached is 30.50 °C Calculate the calorimeter constant. Specific heat of water is 4.184 J/(g-°C). a. 109.4 J/°C b. 551.7 J/°C c. 330.5 J/°C d. 441.1 J/°C e. 220.0 J/°C When 0.250 g of iron (atomic weight = 55.85 g/mol) is burned, 0.341 g of iron oxide is obtained. What is the mass percent of iron in the iron oxide? Given that the atomic weight of Oxygen = 16.00 g/mol. %3D O a. 83.1% O b. 77.9% O c. 75.5% d. 73.3% e. 80.4% In a calorimeter calibration experiment, a sample of 55.50 g of water at 55.00 °C is added to a calorimeter containing 50.50 g of water at 20.00 °C After stirring and waiting for the system to equilibrate, the final temperature reached is 30.50 °C Calculate the calorimeter constant. Specific heat of water is 4.184 J/(g-°C). a. 109.4 J/°C b. 551.7 J/°C c. 330.5 J/°C d. 441.1 J/°C e. 220.0 J/°C