Question

The first part of this experiment involved the calibration of the equipment you will use to measure the rate of oxygen evolution. To do so, you will inject air into the sealed reaction bottle at known temperatures and measure the pressure change within the bottle. Suppose 30.0 mL of air at an initial temperature of 22.5 ºC and an initial pressure of 0.966 atm was injected into a reaction bottle that contained 30.0 mL of water. Use this information to answer the following questions.

(a) How many moles of air are contained in the syringe?
(b) Pretend the gas you injected escaped into the air above the 30.0 mL of water within the vessel. If the gas had remained in the water, what would its "molar concentration" have been?
(c) If the pressure in the flask is observed to be 1.088 atm with no change in temperature after the injection (or after the "escape" from the 30 mL of water in the vessel in our pretend scenario in part B), what is the molar concentration-to-pressure change ratio? This value can be used to convert a change in pressure within the vessel to a molar concentration of gas that escaped from the solution or vice versa. This factor will be used in questions 2 and 3 below.

Answer 1

Step-by-step explanation:

(3 pts) A 5.00 gram sample of an oxide of lead PbxOy contains 4.33 g of lead. Determine the

simplest formula for the compound.