Equal amounts of marble chips are reacted separately with 100cm3 of hydrochloric acid of different concentrations . if all the marble chips reacted, which of the following remained the same in each case? A.Average rate of evolution of gas B.Total mass of gas evolved during the reaction C.Time taken for the reaction to reach completion D.lnitial reaction rates

10 A large excess of marble chips is reacted with 25 cm 3 of 1.0 mol dm –3 hydrochloric acid at 40 C.How is the result different when the reaction is repeated with 60 cm 3 of 0.5 mol dm –3 hydrochloricacid at 40 C?A The reaction is faster and more of the products are made when the reaction is complete.B The reaction is faster and less of the products are made when the reaction is complete.C The reaction is slower and more of the products are made when the reaction is complete.D The reaction is slower and less of the products are made when the reaction is complete.

A student performed an experiment in which they reacted 50cm3 of 0.300mol dm-3 sodium thiosulfate with 5.0cm3 of 2.000 dm-3 hydrochloric acid. They are investigating the affect of changing conditions on the rate of reaction. Which of the following concentrations of hydrochloric acid would result in the slowest rate of reaction?

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

3. A student conducts an experiment where she reacts a lump of zinc (Zn) with hydrochloric acid (HCl). The balanced equation below represents the reaction.     Zn +  2HCl  →  H₂  +  ZnCl₂   Which set of reaction conditions will produce H₂ at the fastest rate?*1.0 g of powdered Zn in 50mL of 1.0 M HCl at 20°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 30°C1.0 g of powdered Zn in 50mL of 1.0 M HCl at 30°Ca 1.0 g lump of Zn in 50mL of 0.5 M HCl at 20°C

In the following first order competing reactionsthe ratio of  k1k2 , if only  94%  of  A  have been reacted whereas  50%  of  C has been reacted, is