The equilibrium constant, K for the following reaction is 2.90x102 at 1.15×10°K. 2503(g)2s0,2(g) + O2(g) If an equilibrium mixture of the three gases in a 11.5 L container at 1.15x10 K contains 0.275 mol of SO,(g) and 0.240 mol of SO, the equilibrium concentration of O, is M.
The equilibrium constant, K for the following reaction is 2.90x102 at 1.15×10°K. 2503(g)2s0,2(g) + O2(g) If an equilibrium mixture of the three gases in a 11.5 L container at 1.15x10 K contains 0.275 mol of SO,(g) and 0.240 mol of SO, the equilibrium concentration of O, is M.
Chemistry
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![The equilibrium constant, \( K_c \), for the following reaction is \( 2.90 \times 10^{-2} \) at \( 1.15 \times 10^3 K \).
\[ 2 \text{SO}_3(\text{g}) \rightleftharpoons 2 \text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \]
If an equilibrium mixture of the three gases in a 11.5 L container at \( 1.15 \times 10^3 K \) contains 0.275 mol of SO₃(g) and 0.240 mol of SO₂(g), the equilibrium concentration of O₂ is _____ M.
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Transcribed Image Text:The equilibrium constant, \( K_c \), for the following reaction is \( 2.90 \times 10^{-2} \) at \( 1.15 \times 10^3 K \).
\[ 2 \text{SO}_3(\text{g}) \rightleftharpoons 2 \text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \]
If an equilibrium mixture of the three gases in a 11.5 L container at \( 1.15 \times 10^3 K \) contains 0.275 mol of SO₃(g) and 0.240 mol of SO₂(g), the equilibrium concentration of O₂ is _____ M.
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![The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.
\[ \text{NH}_4\text{HS(s)} \rightleftharpoons \text{NH}_3\text{(g)} + \text{H}_2\text{S(g)} \]
If an equilibrium mixture of the three compounds in a 7.83 L container at 298 K contains 2.96 mol of \(\text{NH}_4\text{HS(s)}\) and 0.294 mol of \(\text{NH}_3\), the number of moles of \(\text{H}_2\text{S}\) present is:
\[ \underline{\quad\quad\quad\quad\quad\quad\quad\quad} \text{ moles} \]
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Transcribed Image Text:The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.
\[ \text{NH}_4\text{HS(s)} \rightleftharpoons \text{NH}_3\text{(g)} + \text{H}_2\text{S(g)} \]
If an equilibrium mixture of the three compounds in a 7.83 L container at 298 K contains 2.96 mol of \(\text{NH}_4\text{HS(s)}\) and 0.294 mol of \(\text{NH}_3\), the number of moles of \(\text{H}_2\text{S}\) present is:
\[ \underline{\quad\quad\quad\quad\quad\quad\quad\quad} \text{ moles} \]
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