Question

waa r the accepted value at SIF, and the perce REVIEW QUESTIONS MPC, rather than 45 ml of Me would have made any difference in the amount of oxygen was collected? Explain why or why not In this experiment, some oxy en gas will dissolve in water How will this affect the molar volume calculated? Would the molar volume be too high or too low In Step 1, if the outside of flask was wet when you weighed it, how would this affect your results? Would this cause the measured molar volume of oxysen as to be higher or lower? Explain why If 0.65 R of a gas occupies 275 ml at 26 and 1.10 atm, calculate the molar mass of the as 4. S. The density of a gas is 0.980 g/L at 25°C and 365 torr. Calculate the molar mass of the was 6. The density of dry air is 1.2929 g/L at STP Calculate the average molar mass of air. Is this a reasonable value? Explain why or why not. 7. In this experiment, after the reaction went to completion, we let the solutions sit to equill- brate the temperature in flasks A and B. If you did not do this and the gas temperature was too high when you measured the volume of water displaced in the reaction, would the molar volume calculated be too high or too low? Explain why. CAUS 8. Under what conditions do real gases behave most like ideal gases? Does the ait in a room at room temperature (22") and pressure (1 atm) behave ideally? 9. The molar volume for CO, and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these molar volumes slightly less than the ideal molar volume, 22.4 L/mol 10. Hydrogen gas can be produced from the reaction of calcium hydride and water. CaH, (s) + 2 H,O (1) ► 2H2(g) + Ca(OH)2 (aq) How many grams of calcium hydride are needed to produce 2.5 L of hydrogen gas, collected over water at 26°C and 760. torr total pressure?

Answer 1

1.

FeCl₃ acts an a catalyst in the decomposition of Hydrogen Peroxide. It just catalyses the reaction and don't get consumed during the course of the reaction. Amount of oxygen collected will not get affected on changing the amount of FeCl₃ as it doesn't participate in product formation and the amount of oxygen collected will depend on the concentration of hydrogen peroxide.

2.

If some oxygen gets dissolved in the water, moles of oxygen collected will be less. This will affect the molar volume of oxygen which will be too low as a consequence.