Calculate the reaction quotient (Q) for reversible reactions (Formula: Q = [C]c[D]d [A]a[B]b for the reaction aA + bB ⇋ cC + dD)

At a given instant during the reaction $2\text{NO}_{2}(g) \rightleftharpoons \text{N}_{2}\text{O}_{4}(g)$, the concentrations are: $[\text{NO}_{2}] = 0.30 \text{ mol/L}$ and $[\text{N}_{2}\text{O}_{4}] = 0.15 \text{ mol/L}$. Calculate the reaction quotient, $Q$, at this moment.

For the reversible reaction: \(2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)\) At a particular moment, the concentrations are: \([\text{SO}_2] = 0.40\text{ mol L}^{-1}\), \([\text{O}_2] = 0.30\text{ mol L}^{-1}\), and \([\text{SO}_3] = 0.60\text{ mol L}^{-1}\). Determine the reaction quotient, \(Q\), at this moment.

At a particular moment during the reaction $2\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}_2(g)$, the concentrations are: $[\text{NO}] = 0.080 \text{ mol·dm}^{-3}$, $[\text{O}_2] = 0.060 \text{ mol·dm}^{-3}$, and $[\text{NO}_2] = 0.025 \text{ mol·dm}^{-3}$. Calculate the reaction quotient $Q$ at this moment.

At a particular instant during the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, the concentrations are: $[N_2] = 0.48 \text{ mol L}^{-1}$, $[H_2] = 1.20 \text{ mol L}^{-1}$, and $[NH_3] = 0.62 \text{ mol L}^{-1}$. Calculate the reaction quotient, $Q$, for this system. Show your working.