All the reaction between following pairs will produce hydrogen gas, except — Hydrogen Chemistry Question

💡 Solution & Explanation

I need to see the options to provide a complete solution. However, I can explain the general principle: **Principle:** Hydrogen gas is produced when: - Active metals (Li, Na, K, Ca, Mg, Al, Zn, Fe) react with **dilute acids** or **water** - Less active metals do NOT produce $H_2$ with dilute acids **Without seeing options A, B, C, D**, here's the typical pattern: Common pairs that **DO produce** $H_2$: - $Mg + H_2SO_4 \rightarrow MgSO_4 + H_2↑$ - $Na + H_2O \rightarrow NaOH + H_2↑$ - $Zn + HCl \rightarrow ZnCl_2 + H_2↑$ Common pair that **DOES NOT produce** $H_2$: - **Cu + dilute $H_2SO_4$** → No reaction (Cu is below H in reactivity series) - **Cu + dilute HCl** → No reaction - **Ag + HCl** → No reaction **If A is the correct answer**, it likely describes a reaction between: - A **less active metal** (Cu, Ag, Pt, Au) and dilute acid, OR - Two non-metals, OR - An oxidizing acid with a metal that gets oxidized to a higher state without H₂ release **Please provide the options** so I can give the exact explanation for why A specifically does not produce hydrogen gas.