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What happen if potassium chlorate was not completely decomposed?
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How do you figure out how mch oxygen gas escaped when Potassium Chlorate is decomposed in a reation? Also what mass of Potassium
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Here is an example that is worked for you. Just follow the steps.
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potassium chlorate can be thermally decomposed to oxygen and potassium chloride. calculate the mass of potassium chlorate that
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2KClO3 ==> 2KCl + 3O2 You need how many mols O2? That's n = PV/RT. Substitute and solve for n = mols
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how could I determine experimentally whether all the potassium chlorate had been decomposed?
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There may be easier ways to do it but could you dissolve the remainder in water and ppt the chloride
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You know how much oxygen is in the amount KClO3 used in the experiment; measure the oxygen collected
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What volume of oxygen gas will be produced when 13.5 g of potassium chlorate is decomposed at STP?
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per the reaction equation ... each mole of KClO3 produces 1.5 moles of O2 13.5 g / (molar mass
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mols KClO3 = grams/molar mass = ? For every 2 mols KClO3 you get 3 mol O2. 1 mol O2 @ STP occupies
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can anyone help with this problem please.....
Potassium chlorate decomposes according to the following equation: 2KClO3 (s) →
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mols KClO3 = grams/molar mass = ? Using the coefficients in the balanced equation, convert mols
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3 Cl2 + 6 KOH go toKClO3 + 5 KCl + 3 H2O
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A 26.3 gram sample of solid potassium chlorate decomposed and produced 9.45 grams of oxygen gas. What is the percent yield of
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