Post-Laboratory Questions The answers to these questions must be handwritten in
ID: 558364 • Letter: P
Question
Post-Laboratory Questions The answers to these questions must be handwritten in your laboratory notebook and attached to the lab report. shaet the eas of magnesium in each flask was essentially the same, how do you account for the difference 2. In another version of this lab, students ran 4 more experiments by altering amounts of reactants relative to the amounts in Flask 3 (assume 0.50 M Ha was used). Predict the relative change in balloon size, as compared to Flask 3, for the following scenarios. Provide a brief explanation for you predicted change a. Flask 6: The volume of HCl is doubled. b. Flask 7: The concentration of Ha is cut in half.iela c. Flask 8: The amount of magnesium is doubled. (Ioflaks atun d. Flask 8: Both the mass of magnesium and the volume of HCl are doubled. 3. In this lab you investigated how the quantity of gas produced in a reaction changes depending on amounts of starting materials. The same stoichiometric process can be worked but in reverse to answer important questions such as "What amount of magnesium is needed to produce 10 moles of hydrogen gas?". This type of calculation has real world applications, for example, in determining how much of a reactant is needed to produce oxygen gas on the International Space Station. To generate oxygen on the space station, potassium perchlorate (KCIO4) is placed into a metal canister and ignited; oxygen gas is released according to the following unbalanced equation: Ka04(s) Ka(s) + O2(g) On average an astronaut will consume 600 L of oxygen in a day, which is equivalent to 24.5 moles of O2. What mass of potassium perchlorate, in kg, is consumed in a day to generate the needed amount of oxygen for one astronaut?Explanation / Answer
1. For difference in size of the ballons you have to measure the diameter of every ballon , you can use a measuring tape or a ruler, compare the measures.
2. To solve this question you need to provide more information about your experiment, I can see that the reaction you are working with is Mg + 2HCl ==== H2 + MgCl2
please provide mass of magnessium and volume of HCl you used in order to perform limiting reactant calculations, with those calculation we can make predictions
3. the reaction of the statement is incomplete, we need to balance it: you have 4 Oxygens on the left and 2 oxygens on the right, you need to have the same ammount of atoms on each side of the reaction, for this case the easiest thing to do is to multiply by 2 the oxygens on the right so:
KClO4 ======== KCl + 2O2
So 1 mole of KClO4 produces 2 moles of O2, so if you want 24.5 moles of O2 you will need to 24.5/2 = 12.25 moles of KClO4
now we just need to calculate the molar mass of KClO4, O has a molar mass of 16, Cl 35.5 and K 39
so the total molar mass is 39 + 35.5 + 4*16 = 138.5 g/gmol
we know that moles = mass / molar mass
mass = moles * molar mass = 138.5 * 12.25 = 1696.25 grams
divide it by 1000 to get kg ; this is 1.696 Kg or 1.7 kg of KClO4 you need every day
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