An excess amount of zn is added to 500.0 ml of 0.800 m hcl what mass in grams of h2 is produced

Start by writing down the balanced chemical equation that describes this single replacement reaction

#"Zn"_ ((s)) + color(red)(2)"HCl"_ ((aq)) -> "ZnCl"_ (2(aq)) + "H"_(2(g)) uarr#

Now, notice that the two reactants react in a #1:color(red)(2)# mole ratio. This tells you that the reaction will always consume twice as many moles of hydrochloric acid than moles of zinc metal.

As you know, a solution's molarity tells you how many moles of solute, which in your case will be hydrochloric acid, #"HCl"#, are present per liter of solution.

The hydrochloric acid solution is said to have a molarity of #"3.05 mol L"^(-1)#. This means that you get #3.05# moles of hydrochloric acid for every #"1 L"# of solution. Keep this in mind for later.

You know that the reaction must consume #"25.0 g"# of zinc metal. You can convert this mass to moles by using zinc's molar mass

#25.0 color(red)(cancel(color(black)("g"))) * "1 mole Zn"/(65.38color(red)(cancel(color(black)("g")))) = "0.3824 moles Zn"#

In order for this many moles of zinc to react, you'd need

#0.3824 color(red)(cancel(color(black)("moles Zn"))) * (color(red)(2)color(white)(a)"moles HCl")/(1color(red)(cancel(color(black)("mole Zn")))) = "0.7648 moles HCl"#

Since you know that #"1 L"# of your hydrochloric acid solution contains #3.05# moles of hydrochloric acid, ti follows that this many moles would be present in

#0.7648 color(red)(cancel(color(black)("moles HCl"))) * overbrace("1 L solution"/(3.05 color(red)(cancel(color(black)("moles HCl")))))^(color(purple)(" a molarity of 3.05 mol L"^(-1))) = "0.2508 L solution"#

Rounded to three sig figs and expressed in milliliters, the answer will be

#"volume of HCl solution" = color(green)(|bar(ul(color(white)(a/a)"251 mL"color(white)(a/a)|)))#

Note that you have

#"1 L" = 10^3"mL"#

SIDE NOTE The hydrogen gas produced by the reaction will bubble out of solution.

With an understanding of the ideal gas laws, it is now possible to apply these principles to chemical stoichiometry problems. For example, zinc metal and hydrochloric acid (hydrogen chloride dissolved in water) react to form zinc (II) chloride and hydrogen gas according to the equation shown below:

2 HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g)

A sample of pure zinc with a mass of 5.98 g is reacted with excess hydrochloric acid and the (dry) hydrogen gas is collected at 25.0 ˚C and 742 mm Hg. What volume of hydrogen gas would be produced?

This is a “single state” problem, so we can solve it using the ideal gas law, PV = nRT. In order to find the volume of hydrogen gas (V), we need to know the number of moles of hydrogen that will be produced by the reaction. Our stoichiometry is simply one mole of hydrogen per mole of zinc, so we need to know the number of moles of zinc that are present in 5.98 grams of zinc metal. The temperature is given in centigrade, so we need to convert into Kelvin, and we also need to convert mm Hg into atm.

Conversions:

\[25.0\; C+273=298\; K \nonumber \]

\[(742\; mm\; Hg)\times \left ( \frac{1\; atm}{760\; mm\; Hg} \right )=0.976\; atm \nonumber \]

\[(5.98\; g\; Zn)\times \left ( \frac{1.00\; mol}{65.39\; g\; Zn} \right )=0.0915\; mol \nonumber \]

Substituting:

\[PV=nRT \nonumber \]

\[(0.976\; atm)\times V=(0.0915\; mol)(0.0821\; L\; atm\; mol^{-1}K^{-1})(298\; K) \nonumber \]

\[V=\frac{(0.0915\; mol)(0.0821\; L\; atm\; mol^{-1}K^{-1})(298\; K)}{(0.976\; atm)}=2.29\; L \nonumber \]

We can also use the fact that one mole of a gas occupies 22.414 L at STP in order to calculate the number of moles of a gas that is produced in a reaction. For example, the organic molecule ethane (CH3CH3) reacts with oxygen to give carbon dioxide and water according to the equation shown below:

2 CH3CH3 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)

An unknown mass of ethane is allowed to react with excess oxygen and the carbon dioxide produced is separated and collected. The carbon dioxide collected is found to occupy 11.23 L at STP; what mass of ethane was in the original sample?

Because the volume of carbon dioxide is measured at STP, the observed value can be converted directly into moles of carbon dioxide by dividing by 22.414 L mol–1. Once moles of carbon dioxide are known, the stoichiometry of the problem can be used to directly give moles of ethane (molar mass 30.07 g mol-1), which leads directly to the mass of ethane in the sample.

\[(11.23\; L\; CO_{2})\times \left ( \frac{1\; mol}{22.414\; L} \right )=0.501\; mol\; CO_{2} \nonumber \]

Reaction stoichiometry:

\[(0.501\; mol\; CO_{2})\times \left ( \frac{2\; mol\; CH_{3}CH_{3}}{4\; mol\; CO_{2}} \right )=0.250\; mol\; CH_{3}CH_{3} \nonumber \]

The ideal gas laws allow a quantitative analysis of whole spectrum of chemical reactions. When you are approaching these problems, remember to first decide on the class of the problem:

If it is a “single state” problem (a gas is produced at a single, given, set of conditions), then you want to use PV = nRT.
If it is a “two state” problem (a gas is changed from one set of conditions to another) you want to use \[\frac{P_{1}V_{1}}{n_{1}T_{1}}=\frac{P_{2}V_{2}}{n_{2}T_{2}} \nonumber \]
If the volume of gas is quoted at STP, you can quickly convert this volume into moles with by dividing by 22.414 L mol-1.

Once you have isolated your approach ideal gas law problems are no more complex that the stoichiometry problems we have addressed in earlier chapters.

An automobile air bag requires about 62 L of nitrogen gas in order to inflate. The nitrogen gas is produced by the decomposition of sodium azide, according to the equation shown below

2 NaN3 (s) → 2 Na (s) + 3 N2 (g)

What mass of sodium azide is necessary to produce the required volume of nitrogen at 25 ˚C and 1 atm?

When Fe2O3 is heated in the presence of carbon, CO2 gas is produced, according to the equation shown below. A sample of 96.9 grams of Fe2O3 is heated in the presence of excess carbon and the CO2 produced is collected and measured at 1 atm and 453 K. What volume of CO2 will be observed?

2 Fe2O3(s) + 3 C (s) → 4 Fe (s) + 3 CO2 (g)

The reaction of zinc and hydrochloric acid generates hydrogen gas, according to the equation shown below. An unknown quantity of zinc in a sample is observed
to produce 7.50 L of hydrogen gas at a temperature of 404 K and a pressure of 1.75 atm. How many moles of zinc were in the sample?

Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2 (g)