A fixed number of moles of monatomic ideal gas is initially in a state where the pressure is 110 kPa and the volume is 0.700 liters. Then, the temperature of the gas is doubled, by the following two-step process. First, there is a constant-volume process that brings the pressure to (8/5) of the original pressure. This is followed by a constant-pressure process that increases the volume of the gas until the temperature is double the temperature in the initial state (specified in the first sentence of this part). Calculate the net work done by the gas in this two-step process.

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.)