Chemistry
13th Edition
ISBN: 9781260162370
Author: Chang
Publisher: MCG
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Chapter 22, Problem 22.105QP
Assuming ideal behavior, calculate the density of gaseous HF at its normal boiling point (19.5°C). The experimentally measured density under the same conditions is 3.10 g/L. Account for the discrepancy between your calculated value and the experimental result.
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Students have asked these similar questions
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
L-atm
on experimentally collected data, the student calculates R to equal 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 =
%
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but
does not dislodge it.
The student does not clean the zinc metal with sand paper.
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 uses the barometric pressure for the lab to calculate R.
1. The partial pressure of oxygen is 0.20 atm at sea level at 25°C. Calculate its
partial pressure at an altitude of 30 km (the stratosphere).
From two moles of molten tin whose temperature at a
constant pressure of latm has quickly reached 495k.
1771 joules are heated. Determine how many moles of tin
have solidified under these conditions (pressure 1atm and
temperature 495k)?
ΔΗ
T0T0 Jlmel
Imon =505 K
cp 12,5 26 x 1o T JImol
2,2x10 T Jmol
Chapter 22 Solutions
Chemistry
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