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The heat of combustion of propanol (C3H9O) at 298.15 K, determined in a bomb
calorimeter is 43.5 kJ/g. For the combustion of one mole of propanol, determine ΔH
(kJ/mol)?
What is the wavelength of spectral line resulted from the electron transition from n=3
to n=1 in a hydrogen atom?
A gas mixture that has the following composition in percent by volume: 10.2% CO2,
21.0% CO, 18.5% H2, 2.3% CH4 and 48.0% N2.
(a) What is the density of this gas at 24 °C and 755 mmHg, in grams per liter?
(b) What is the partial pressure of CO in this mixture at STP?
(c) What volume of air is required for the complete combustion of this mixture of gas? (Air
contains 21% O2 by volume)
3.6 g of an inorganic metal oxide ore mainly contains 90% of Nickel (III) oxide which
decomposes to elemental nickel and oxygen gas. Produced 880 mL of oxygen were
collected over water at a temperature of 25 °C with a total pressure of 747 mmHg. What
is the percent yield of decomposition reaction? (PH2O:23.7 mmHg at 25 °C)
A) A 3.2 g of unknown fluorocarbon compound is decomposed at 298K and produced
310 mL of fluorine gas (F2) is collected over water at 25 °C. What is the percent Fluorine
by mass in this unknown fluorocarbon compound [The vapor pressure of water at 25 °C
is 23.76 mmHg]
B) When 1 mole of this fluorocarbon compound was completely combusted in a bomb
calorimeter, it liberates 3870 kJ of heat which causes the temperature to increase from
25 °C to 26.5 °C. Compute the heat capacity of the bomb calorimeter?
When 1 mole of this fluorocarbon compound was completely combusted in a bomb
calorimeter, it liberates 3870 kJ of heat which causes the temperature to increase from
25 °C to 26.5 °C. Compute the heat capacity of the bomb calorimeter?
A 3.2 g of unknown fluorocarbon compound is decomposed at 298K and produced
310 mL of fluorine gas (F2) is collected over water at 25 °C. What is the percent Fluorine
by mass in this unknown fluorocarbon compound [The vapor pressure of water at 25 °C
is 23.76 mmHg]
How many grams of O2 is produced when 30 g of potassium chlorate decomposes with the 72% yield.
KClO3 → KCl + O2
Assume that produced O2 is collected in a container, and it is pressure suddenly released
from 6.2 atm to 2.3 atm at 30°C. How much work, in joules, is done during this process?
A researcher tries to find out the mass percent composition of an Iron ore sample.
The researcher weighted 1.30 g of Iron ore and dissolved it in HCl (aq) solution. Based on
the given redox reaction generated Fe2+ is titrated with 32.5 mL of 0.088 M of potassium
permanganate. Find the mass percent Fe in the ore sample? What if the researcher dilutes
the potassium permanganate solution to half and uses the same volume of solution for
titration, how many grams of iron remains unreacted?
Fe2+ + MnO4- → Fe3+ + Mn2+ (not balanced)
A company uses H2 gas to generate electricity. They studied a smaller scale model
reaction to figure out the maximum amount of H2 gas that they can produce. For this
purpose, they used an alloy consisting of 95% Al by mass. The alloy has a density of 3.12
g/cm3 and they took a 0.875 cm3 small piece of alloy to react with 200 mL of 1.2 M solution
of HCl based on the given Al specific reaction. What is the maximum amount of H2 gas
that can be produced? What are the limiting and remaining reagents? How can they
increase the amount of H2 gas that they obtained?
Al + HCl → AlCl3 + H2 (not balanced)
