Mg3N2 + 6H20 = 3Mg(OH) + 2NH3
What mass of magnesium nitride would you need to react with excess water to produce 25g of ammonia?
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Mg, N2(8) + 6H2O(l) + 3Mg(OH)2(aq) + 2NH3(aq) If 4 moles of magnesium nitride react, The reaction consumes The reaction produces moles of water. moles of magnesium hydroxide and moles of ammonia.
please show work? Question 32 (8 points) What mass of NH3 is formed when 9.32 g of Mg3N2 reacts with water according the equation? Mg3N2 + 6H20 3Mg(OH)2 + 2NH3 Please report your answer to the correct number of significant figures. Leave a space between the number and the unit.
Mg3N2+6H2O->3Mg(OH)2+2NH3 When 2 moles of Mg3N2 are allowed to react, how many miles of H2O also react?
Uuel Score: 1.50/ Autos Tutored Practice Problem 8.2.4 COUNTS TOWARDS GRADE Use reaction stoichiometry to calculate amounts of reactants and products. Close Problem The substances magnesium nitride and water react to form magnesium hydroxide and ammonia. Unbalanced equation: Mg3N2 (5) + H20 (1) Mg(OH)2 (aq) + NH3 (aq) In one reaction, 66.4 g of NH, is produced. What amount (in mol) of H20 was consumed? What mass (in grams) of Mg(OH)2 is produced? mol H2O consumed g Mg(OH)2 produced Check...
If water is added to magnesium nitride, ammonia gas is produced when the mixture is heated. Mg3N2(s) + 3 H20(1)→ 3 MgO(s) + 2 NH3(g) If 11.7 g of magnesium nitride is treated with water, what volume of ammonia gas would be collected at 28°C and 739 mm Hg?
2)how many moles of barium sulfate are sulfate are produced from 0.1 mole of barium chloride? b) 3 moles of BACL2 will react to produce how many moles of potassium chloride? and so on..... 2) For the balanced equation; BaCl2 + K2SO4 → BaSO4 + 2KCI a) How many mole(s) of barium sulfate are produced from 0.1 mole of barium chloride? b) 3 moles of BaCl2 will react to produce how many moles of potassium chloride? 3) For the balanced...
Magnesium and nitrogen react in a combination reaction to produce magnesium nitride. 3 Mg + N2 → Mg3N2. In a particular experiment, a 9.27 g sample of N2 reacts completely. The mass of Mg consumed is ___________g. a. 8.04 b. 24.1 c. 16.1 d. 0.92 e. 13.9
How many grams of N2 are produced from 100.0 g of NH3 according to the following reaction? 4NH3 + 6NO ------ > 5N2 + 6H20 Calculate the mass (g) of H2O needed to produce 150 g of Mg(OH)2 according to the equation: Mg2N2 + 6H2O ----- > 3Mg(OH)2 + 2NH3
For the following reaction, 4.79 grams of magnesium nitride are mixed with excess water. The reaction yields 6.84 grams of magnesium hydroxide. magnesium nitride (s) + water (l) magnesium hydroxide (aq) + ammonia (aq) What is the theoretical yield of magnesium hydroxide? grams What is the percent yield for this reaction? %
For the following reaction, 5.18 grams of water are mixed with excess magnesium nitride. The reaction yields 6.10 grams of magnesium hydroxide. magnesium nitride (s) + water (l) -> magnesium hydroxide (aq) + ammonia (aq) What is the ideal yield of magnesium hydroxide? grams What is the percent yield for this reaction? %