A 0.500 g sample of TNT (C2H5N206) is burned in a bomb calorimeter containing 610 grams of water at an initial temperature of 20.0°C. After the reaction, the final temperature of the water is
22.7°C. The heat capacity of the calorimeter is 420 J/°C.
How much heat was produced in the combustion of TNT?
A. 3374kJ
B. 8.04kJ
C. 2.97kJ
D. 8025 kJ
E. 3.37kJ
Was the heat released or absorbed by the water and calorimeter?
A. Absorbed
B. Released

What is the most stable monatomic ion formed from nitrogen

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

In 1901, thomas edison invented the nickel-iron battery. the following reaction takes place in the battery. fe(s) + 2 nio(oh)(s) + 2 h2o(l) fe(oh)2(s) + 2 ni(oh)2(aq) how many mole of fe(oh)2, is produced when 5.35 mol fe and 7.65 mol nio(oh) react?