1. When ferric sulfide is roasted in oxygen, solid ferric oxide and sulfur dioxi

Question

1. When ferric sulfide is roasted in oxygen, solid ferric oxide and sulfur dioxide gas are formed. Write out the balanced chemical reaction for the roasting. How many liters of pure oxygen gas are needed at 55oC and 748 mm Hg to react completely with 2.20 kg of ferric sulfide? How many liters of dry air (Hint: Table 6.1) would you need to do the same reaction?

2. At 273.15 K and 1.0 atm, 1.0 L of some gas contains C, H and N. The gas combusts to give 2.0 L CO2, 3.5 L of H2O, and 0.50 L of N2. What is the empirical formula?

3. A gas mixture with 321 mg of methane, 175 mg of argon and 225 mg of nitrogen was made and placed in a balloon. The partial pressure of nitrogen in the mixture at 311 K is 15.7 kPa. What is the volume of the balloon (in liters)? What is the total pressure (in kPa) of the mixture?

4. (words not numbers for this problem) At 375 K, gas tank 1 and gas tank 2 each contain 3 moles of gas. Tank 1 has carbon monoxide. Tank 2 has helium. Compare (which tank is higher or lower)

A. the kinetic energy of the molecules.

B. the velocity of the molecules.

C. The time it would take the molecules to effuse out.

Explanation / Answer

1. When ferric sulfide is roasted in oxygen, solid ferric oxide and sulfur dioxi

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