In a series of experiments controlled, a researcher reacted portions of 3,27g of

Question

In a series of experiments controlled, a researcher reacted portions of 3,27g of metallic zinc with different volumes Hydrochloric acid solutions of different titles, according to the following equation:

2 HCl + Zn ------> ZnCl2 + H2

If, in the various experiments made, are kept constant mass and state aggregation of zinc and also the temperature and pressure under which these experiments are performed, check the option that describes the conditions under which it may be observed most reaction speed.

a) Experiment I: Solution 2000ml HCl containing 1,825g / L + Zn

b) Experiment II: Solution 1000ml HCl containing 3,65g / L + Zn

c) Experiment III: Solution 500mL HCl containing 7,30g / L + Zn

d) Experiment IV: Solution 250mL HCl containing 14,60g / L + Zn

Make the statement calculate your answer. (Explain passes by step)

Explanation / Answer

From the equation, 2 mols of HCl reacts with 1 mole of Zn metal

moles of Zn started with = 3.27 g/65.38 g/mol = 0.05 mol

So moles of HCl required would be for complete reaction = 2 x 0.05 = 0.1 mol

a) moles of HCl = (1.825 g/36.5 g/mol) x 2 L = 0.1 mol

b) moles of HCl = (3.65 g/36.5 g/mol) x 1 L = 0.1 mol

c) moles of HCl = 0.1 mol

d) moles of HCl = 0.1 mol

So in all we have equal number of moles of HCl present. The reaction will be fastest in lowest volume.

So, In

d) Experiment IV: Solution 250mL HCl containing 14,60g / L + Zn

reaction would be fastest.

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