Q3: Ammonia can be made by reaction of water with magnesium nitride: __ Mg3N2(s) + __ H2O(l) -> __ Mg(OH)2(s) + __ NH3(g) When the equation is properly balanced, the sum of the coefficients is A) 6 B) 14 C) 12 D) 9 E) 8 Q4: Which one of the following compounds is a strong electrolyte? a) CH3COOH b) C6H12O6 c) NH4Br d) NH3 e) CH3CH2OH Q5: How many grams of AgCl (molar mass = 143.3 g/mol) will be formed if 25.00 mL of 0.450 M AgNO3 solution completely react with excess NaCl solution? AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq) a) 2.69 g b) 2.33 g c) 1.97 g d) 1.61 g e) 1.25 g
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The sum of the coefficients is 3+12+6+6 = 27. However, this option is not available in the choices. There might be a mistake in the question or the choices. Q4: A strong electrolyte is a substance that completely, or almost completely, ionizes or dissociates in Show more…
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Ammonia can be made by reaction of water with magnesium nitride as shown by the following unbalanced equation: Mg 3N 2( s) + H 2O( l) → Mg(OH) 2( s) + NH 3( g) If this process is 81% efficient, what mass of ammonia can be prepared from 23.0 kg magnesium nitride? a. 3.1 kg NH3 b. 6.3 kg NH3 c. 3.9 kg NH3 d. 19 kg NH3 e. 7.8 kg NH3
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Magnesium nitride is a green ionic solid that reacts with water: Mg3N2 + 6H2O = 3Mg(OH)2 + 2NH3 (a) Predict the amount of magnesium nitride required to produce 1.5 mol of ammonia. (b) Predict the amount of water required to produce 1.5 mol of ammonia. (c) What amount of magnesium nitride is required to react completely with 0.25 mol of water? What amounts of the products are expected?
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The fertilizer, ammonium nitrate, is made by reacting ammonia with nitric acid. (Section $1.4)$ (a) Write a balanced equation, with state symbols, for the reaction of ammonia gas with nitric acid to form a solution of ammonium nitrate. (b) Rewrite the equation to show the ions present in the reactants and products, and hence write an ionic equation for the reaction. (c) What type of chemical reaction does your equation represent? Nitric acid is manufactured from ammonia. The first stage in this process involves burning ammonia in oxygen on the surface of a platinum gauze catalyst. The products are $\mathrm{NO}$ and $\mathrm{H}_{2} \mathrm{O}$. (d) Construct a balanced equation for the buming of $\mathrm{NH}_{3}$ in $\mathrm{O}_{2}$. (o) Calculate the maximum mass of NO that could be obtained by burning $1.00 \mathrm{kg}$ of $\mathrm{NH}_{3}$ and the mass of oxygen required. (f) In practice, $1.45 \mathrm{kg}$ of $\mathrm{NO}$ were obtained from the reaction in (e). What was the percentage yield of the reaction?
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