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25. A 10.0 g sample containing calcium carbonate and an inert material was placed in excess hydrochloric acid. A reaction occurred producing calcium chloride, water, and carbon dioxide. (a) Write a balanced equation for the reaction. (b) When the reaction was complete, 1.55 g of carbon dioxide gas was collected. How many moles of calcium carbonate were consumed in the reaction? (c) If all the calcium carbonate initially present in the sample was consumed in the reaction, what percent by mass of the sample was due to calcium carbonate? (d) If the inert material was only silicon dioxide, what was the mole fraction of silicon dioxide in the mixture? mole fraction = N1  n1 n total (e) In fact perhaps there had been some other material present in the original sample that was not so inert and generated a gas during the reaction. Would this have caused the calculated percentage of calcium carbonate in the sample to be higher, lower or have no effect? Justify your response.

25. A 10.0 g sample containing calcium carbonate and an inert material was placed in excess hydrochloric acid. A reaction occurred producing calcium chloride, water, and carbon dioxide.
(a) Write a balanced equation for the reaction.
(b) When the reaction was complete, 1.55 g of carbon dioxide gas was collected. How many moles of calcium carbonate were consumed in the reaction?
(c) If all the calcium carbonate initially present in the sample was consumed in the reaction, what percent by mass of the sample was due to calcium carbonate?
(d) If the inert material was only silicon dioxide, what was the mole fraction of silicon dioxide in the mixture? mole fraction = N1  n1 n total
(e) In fact perhaps there had been some other material present in the original sample that was not so inert and generated a gas during the reaction. Would this have caused the calculated percentage of calcium carbonate in the sample to be higher, lower or have no effect? Justify your response. 

Grade:11

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