150 mL of hydrochloric acid of the same concentration is poured into each of two flasks (A and B).10 g of magnesium (Mg) is added to each flask.Bubbles of hydrogen gas are seen in each flask. The reaction in flask A stops sooner than in flask B.When the bubbling in both flasks stops, no solid magnesium is visible in either flask.Question promptWhat is the balanced chemical equation for this reaction?Question response areaSelect one optionMg + 2HClMgCl2 + H22Mg + 2HCl2MgCl + 2H2Mg + HClMgCl + H22Mg + 2HCl2MgCl + H2

Magnesium metal reacts with hydrochloric acid. At the end of the reaction there is a small amount of magnesium left at the bottom of the flask. Which of the reactants was the limiting reactant?

1.00 g of magnesium ribbon reacted with 25.0 cm3 of 1.00 mol dm–3 hydrochloric acid. Determine the volume, in cm3, of a balloon filled with the hydrogen gas produced at SATP (25°C and 100 kPa).                Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)1018 cm3619 cm3450 cm3310 cm3

Ex 1:Hydrochloric acid reacts with magnesium hydroxide to producewater and aqueous magnesium chloride. How much water isproduced if 20.0 g of hydrochloric acid reacts with 10.0 g ofmagnesium hydroxide? How much of the excess reactant is leftover?

Write the balanced equation for the following chemical reactions.(i) Hydrogen + Chlorine → Hydrogen chloride(ii) Barium chloride + Aluminium sulphate → Barium sulphate + Aluminium chloride(iii) Sodium + Water → Sodium hydroxide + Hydrogen

The balanced symbol equation for the reaction between magnesium and hydrochloric acid is shown below.When writing the ionic equation the ions present in the reaction need to be identified, in the reactants and products.Match the reactants and products to the ions and descriptions. HydrogenMagnesium chlorideMagnesiumHydrochloric acidPossible AnswersI DON'T KNOWRESETSUBMIT ANSWER