\( \quad \) Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 705 K : \[ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \] When she introduced 0.0389 moles of \( \mathrm{N}_{2}(g) \) and 0.0706 moles of \( \mathrm{H}_{2}(g) \) into a 1.00 liter container, she found the equilibrium concentration of \( \mathrm{H}_{2}(g) \) to be 0.0680 M . Calculate the equilibrium constant, \( K_{\mathrm{c}} \), she obtained for this reaction. \( K_{\mathrm{c}}= \)

б) \( \sum_{i=1}^{\infty} \frac{1}{i(i+1)} \)

\( \begin{aligned} & =5.67 \\ \text { 2. } & \text { Debt-to-Equity Ratio }=\text { Total Liabilities } / \text { Total Equity } \\ & =360,000 \text { Baht } / 2,445,000 \text { Baht } \\ & =0.15\end{aligned} \)

e number of electrons that can saturate each energy level an atom equals a) three times the energy level number. b) twice the square of the energy level number. c) twice the energy level number. d) twice the cube of the energy level number.

experimental plant after \( x \) days can be an represented by the formula \( 3(4 x+2) \). The height of a second plant can be repreverted by the formula \( 6(2 x+2) \). is it possible that the two plants will ever be the same height? taplain.

Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 656 K : \[ 2 \mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \] When she introduced 0.0830 moles of \( \mathrm{NH}_{3}(g) \) into a 1.00 liter container, she found the equilibrium concentration of \( \mathrm{H}_{2}(g) \) to be 0.114 Calculate the equilibrium constant, \( K_{\mathrm{c}} \), she obtained for this reaction. \( K_{\mathrm{c}}=\square \)