When heated, KClO3 solid forms solid KCl and O2 gas. A sample of KClO3 is heated and 365 mL of gas with a pressure of 790 mmHg is collected over water, at 26 ∘C. At 26 ∘C, the vapor pressure of water is 25 mmHg: 2(KClO3)(s)→2(KCl)(s)+3(O2)(g)
Part A
What is the pressure of the dry O2 gas?
Express your answer with the appropriate units.
PO2 = ??
Part B
How many moles of O2 were produced?
Express your answer with the appropriate units.
n =
Part C
How many grams of KClO3 were reacted?
Express your answer with the appropriate units.
m = ???
1
Expert's answer
2015-11-04T09:45:11-0500
2KClO3(s)→2KCl(s)+3O2(g) Part A. The total pressure over water consist of the partial pressures of oxygen and water vapour: P(total) = P(oxygene)+P(vapour); P(oxygene) = P(total) - P(vapour) = 790 – 25 = 765 mmHg OR 1.007 atm OR 101992 Pa Part B. The number of moles of oxygen can be calculated using the formula of ideal gas law converting the values to SI units - V = 0.000365 m3 ; T = 299.15 K; R = 8.314 J/(mol*K):
The number of moles using the selected equation is n = 0.015 mole. Part C. The number of moles of KClO3 is 0.015x2/3 = 0.01 mole The molar mass of KClO3 is122.55 g/mol The mass of KClO3 is m = nM = 0.01x122.55 = 1.225 g
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28.04.20, 19:38
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27.04.20, 19:44
Solid aluminum reacts with aqueous H2SO4 to form H2 gas and aluminum
sulfate. When a sample of Al is allowed to react, 680 mL of gas is
collected over water at 23 ∘C, at a pressure of 745 mmHg . At 23
∘C, the vapor pressure of water is 21 mmHg:
2Al(s)+3H2SO4(aq)→3H2(g)+Al2(SO4)3(aq) What is the pressure of the
dry H2 gas? How many moles of H2 were produced? How many grams of Al
were reacted?
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Dear Matias, Questions in this section are answered for free. We can't fulfill them all and there is no guarantee of answering certain question but we are doing our best. And if answer is published it means it was attentively checked by experts. You can try it yourself by publishing your question. Although if you have serious assignment that requires large amount of work and hence cannot be done for free you can submit it as assignment and our experts will surely assist you.
Solid aluminum reacts with aqueous H2SO4 to form H2 gas and aluminum sulfate. When a sample of Al is allowed to react, 680 mL of gas is collected over water at 23 ∘C, at a pressure of 745 mmHg . At 23 ∘C, the vapor pressure of water is 21 mmHg: 2Al(s)+3H2SO4(aq)→3H2(g)+Al2(SO4)3(aq) What is the pressure of the dry H2 gas? How many moles of H2 were produced? How many grams of Al were reacted?
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