Question

2. Arnie is going to dissolve 2.65g of zinc using 6.0M hydrochloric acid. A) what volume of the acid will he need to dissolve all the zinc? B) He wants to collect the gas produced by the reaction in a container, determine the volume of container he will need if the pressure is 628 mmHg and temperature is 23ᵒC. C) What is the mass of the zinc chloride he will produce? You will need a balanced equation and a gas law for this question.

Answer 1

Answer:

Explanation:

Zn + 2HCl = ZnCl₂ + H₂

A ) mole of Zn = 2.65 / 65

= .04 mol

mole of HCl required = .04 x 2 mol

.08 mol

If v be the volume required

v x 6 = .08

v = .0133 liter

= 13.3 cc

B )

volume of gas at NTP :

moles of gas  obtained = .04 moles

= 22.4 x .04 liter

= .896 liter

we have to find this volume at given temperature and pressure

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

$\frac{760\times.896}{273} =\frac{628\times V_2}{296}$

$V_2$ = 1.175 liter.

C )

.04 mole of zinc chloride will be produced

mol weight of zinc chloride

= 65 + 35.5 x 2

= 136 gm

.04 mole = 136 x .04

= 5.44 gm