1. Detonation of nitroglycerin proceeds as shown in the following equation.
4 C3H5O9N3(l) → 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g)
(a) If a sample containing 1.97 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how many total moles of gas are produced?
(b) If each mole of gas occupies 43 L under the conditions of the explosion, how many liters of gas are produced?
(c) How many grams of N2 are produced in the detonation?
2. One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO.
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
In a certain experiment, 2.10 g of NH3 reacts with 3.44 g of O2.
a) How many grams of the excess reactant remains after the limiting reactant is completely consumed?
3. Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4·x H2O, where x indicates the number of moles of H2O per mole of MgSO4. When 5.469 g of this hydrate is heated to 250°C, all the water of hydration is lost, leaving 2.671 g of MgSO4. What is the value of x? MAKE SURE IT IS IN THE CORRECT SIG DIG