216. Considering the following thermochemical reactions: (I) $\text{CS}_2(\text{l}) + \text{O}_2(\text{g}) \rightarrow \text{CO}_2(\text{g}) + \text{SO}_2(\text{g})$ $\Delta H = -1075\ \text{kJ}$ (II) $\text{NH}_3(\text{g}) + \text{O}_2(\text{g}) \rightarrow \text{N}_2(\text{g}) + \text{H}_2\text{O}(\text{l})$ $\Delta H = -1530\ \text{kJ}$ (equations are balanced) The heat of combustion of each gram of ammonia is equal to the heat of combustion of how many grams of carbon disulfide, and how many moles of gas are produced per mole of ammonia burned in reaction (II)? (Read the options from right to left.) $(H = 1,\ C = 12,\ N = 14,\ S = 32 : \text{g.mol}^{-1})$ (1) $5/\!0\ ,\ 1/\!59$ (2) $2\ ,\ 2/\!19$ (3) $1\ ,\ 1/\!59$ (4) $2/\!25\ ,\ 2/\!19$
\textbf{216.} Considering the following thermochemical reactions:
(I) $\text{CS}_2(\text{l}) + \text{O}_2(\text{g}) \rightarrow \text{CO}_2(\text{g}) + \text{SO}_2(\text{g})$ \quad $\Delta H = -1075\ \text{kJ}$
(II) $\text{NH}_3(\text{g}) + \text{O}_2(\text{g}) \rightarrow \text{N}_2(\text{g}) + \text{H}_2\text{O}(\text{l})$ \quad $\Delta H = -1530\ \text{kJ}$ (equations are balanced)
The heat of combustion of each gram of ammonia is equal to the heat of combustion of how many grams of carbon disulfide, and how many moles of gas are produced per mole of ammonia burned in reaction (II)? (Read the options from right to left.)
$(H = 1,\ C = 12,\ N = 14,\ S = 32 : \text{g.mol}^{-1})$
(1) $5/\!0\ ,\ 1/\!59$ \quad\quad (2) $2\ ,\ 2/\!19$
(3) $1\ ,\ 1/\!59$ \quad\quad (4) $2/\!25\ ,\ 2/\!19$