Express in grams. All measurements in stp.
(A) 0.4 moles of sodium sulphate.
(B) 1.12 litres of HCl.
Answers
Answer:
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)
Example 9.6.1 :
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?
Solution
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:
25.0C+273=298K(9.6.1)
(742mmHg)×(1atm760mmHg)=0.976atm(9.6.2)
(5.98gZn)×(1.00mol65.39gZn)=0.0915mol(9.6.3)
Substituting:
PV=nRT(9.6.4)
(0.976atm)×V=(0.0915mol)(0.0821Latmmol−1K−1)(298K)(9.6.5)
V=(0.0915mol)(0.0821Latmmol−1K−1)(298K)(0.976atm)=2.29L(9.6.6)
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)
Example 9.6.1 :
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?
Solution
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.
(11.23LCO2)×(1mol22.414L)=0.501molCO2(9.6.7)
Reaction stoichiometry:
(0.501molCO2)×(2molCH3CH34molCO2)=0.250molCH3CH3(9.6.8)
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
P1V1n1T1=P2V2n2T2(9.6.9)
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