A sample of magnesium nitride (Mg3N2\text{Mg}_3\text{N}_2Mg3N2) was reacted completely with water to produce ammonia gas, NH3\text{NH}_3NH3, according to the following equation:
Mg3N2(s)+6H2O(l)→3Mg(OH)2(s)+2NH3(g) \text{Mg}_3\text{N}_2(\text{s}) + 6\text{H}_2\text{O}(\text{l}) \rightarrow 3\text{Mg(OH)}_2(\text{s}) + 2\text{NH}_3(\text{g}) Mg3N2(s)+6H2O(l)→3Mg(OH)2(s)+2NH3(g)The volume of ammonia gas collected was 120.0 cm3 at a temperature of 298 K and a pressure of 98.0 kPa.
What is the amount, in moles, of magnesium nitride that reacted?
The gas constant, R=8.31 J K−1 mol−1R = 8.31\text{ J K}^{-1}\text{ mol}^{-1}R=8.31 J K−1 mol−1
2.37×10−62.37 \times 10^{-6}2.37×10−6
2.37×10−32.37 \times 10^{-3}2.37×10−3
4.75×10−34.75 \times 10^{-3}4.75×10−3
9.50×10−39.50 \times 10^{-3}9.50×10−3