Question

1. Solid zinc was added to 1.0L of 0.100 M HCl and the following data were generated:

Time (seconds)	Mass of Zn (g)
0	0.016
4	0.014
8	0.012
12	0.010
16	0.008

a) Write a balanced chemical equation for this reaction.

b) Find the rate of reaction in moles of Zn consumed per time (units of moles/s)

c) Write the complete NET IONIC equation for this equation. (If you need help with writing a net ionic equation, see this video here)

d) What will happen as the [H+] decreases?

e) What will happen as the [Cl-] decreases?

Answer 1

a) Balanced chemical equation – Zn(s) +2H Cd (aq) → Znch (aq) + H₂ (g) (b) Initial moles of Zn = 0.016 - Cat t=o) 65 moles of zinc at tot = 0.014 "(t=4) 65 Rate of reaction (mol(s) :-( ovome -0.016) 65 4- 0 = 0.002 6584 = 7.692 x10-6 molls (c) Net ionic equation - 2068) + 2H+ (aq) + 2C* (aq) → zat cap) +28[+ 2H(4) Zn(s) + 2H+ (aq) → Zn2+ (aq) + 2H, (0) CH+ ] decrease then moles of Zn2+ and H₂ produced will be decrease. (E) [ae ] decrease, it has no impact on reaction,

Rate of the reaction = 7.692 × 10 -6 mol/s