Al in I1-42. Sodium reacts with anhydrous ammonia to produce sodium amide, NaNH,(s). How many grams of sodium amide can be produced from 10.0 grams 4. of sodium? 11-50. Phosphorus forms a compound similar to am- monia. The compound has the chemical formula PH, and is called phosphine. It can be prepared by the reaction described by the equation P,(s) + 3 NAOH(aq) + 3 H,O (1) → PH,(g) +3 NaH,PO,(aq) If 20.0 grams of phosphorus and a solution contain- ing 50.0 grams of NaOH are reacted with H,O(1) in excess, how many grams of phosphine will be ob- tained?

Al in I1-42. Sodium reacts with anhydrous ammonia to produce sodium amide, NaNH,(s). How many grams of sodium amide can be produced from 10.0 grams 4. of sodium? 11-50. Phosphorus forms a compound similar to am- monia. The compound has the chemical formula PH, and is called phosphine. It can be prepared by the reaction described by the equation P,(s) + 3 NAOH(aq) + 3 H,O (1) → PH,(g) +3 NaH,PO,(aq) If 20.0 grams of phosphorus and a solution contain- ing 50.0 grams of NaOH are reacted with H,O(1) in excess, how many grams of phosphine will be ob- tained?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....

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Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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