EP GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
11th Edition
ISBN: 9780133897340
Author: Petrucci
Publisher: PEARSON CO
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Question
Chapter 6, Problem 95IAE
Interpretation Introduction
Interpretation:
The molecular formula of compound should be determined.
Concept introduction:
The ideal gas equation gives the relationship between P, V, n and T. It is the combination of different
Where, P = pressure
V = volume
n = number of moles (ratio of mass to the molar mass)
R = Universal gas constant
T = temperature
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A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1.
a) How many moles of propane are in the cylinder?
b) What is the mass of the propane inside the cylinder?
c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the
cylinder after it has cooled?
A student experimentally determines the gas law constant, R, by reacting a small piece of
magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water
in a eudiometer. Based on experimentally collected data, the student calculates R to equal
L'atm
0.0832
mol·K
L'atm
Ideal gas law constant from literature: 0.08206
mol·K
(a) Determine the percent error for the student's R-value.
Percent error =|1.389
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student uses the barometric pressure for the lab to calculate R.
The student does not equilibrate the water levels within the eudiometer and the
beaker at the end of the reaction. The water level in the eudiometer is 1-inch
above the water level in the beaker.
The student does not clean the zinc metal with sand paper.
The student notices a large air bubble in the eudiometer after collecting the
hydrogen gas, but does not dislodge it.
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was
the mole fraction of each gas in the mixture? Assume complete combustion.
Xmethane =
Xpropane
Chapter 6 Solutions
EP GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
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