Concept explainers
Interpretation:
Molecular formula of the compound with
Concept Introduction:
An ideal gas contains a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is a theoretical concept. Gases that show perfect elastic collision are practically not possible. At higher
Here,
Empirical formula represents simplest positive integer ratio of atoms in the compound. It only gives proportions of elements in compound. Molecular formula consists of chemical symbols for the respective elements followed by numeric subscript that denotes the number of atom of each element present in molecule.
Answer to Problem 3B.39E
Chemical formula of hydrocarbon is
Explanation of Solution
Replace all
The expression to relate number of moles, mass and molar mass of
Substitute
The expression to relate number of moles, mass and molar mass of
Substitute
The expression to relate number of moles, mass and molar mass of
Substitute
Preliminary formula for compound is formed with moles of
Each of subscript of
The conversion factor to convert
Expression for ideal gas equation is as follows:
Rearrange equation (4) to calculate
Substitute
The expression to relate number of moles, mass and molar mass of
Rearrange in equation (6) to calculate molar mass of
Substitute
Mass from empirical formula can be calculated as follows:
Molar mass and empirical formula are related by formula as follows:
Rearrange equation (8) to calculate
Substitute
Molecular formula of the compound that has
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Chapter 3 Solutions
Chemical Principles: The Quest for Insight
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- Elemental analysis of an organic liquid with a fishy odour gives the following elemental mass percentages: H 14.94 % C 71.22% N 13.84 %. Vaporization of 270 mg of an impure sample in a 150-mL bulb at 150oC gives a pressure of 435 torr. What is the molecular formula of the compound, and the % purity of the sample?arrow_forwardAt 1°C a 1.0-L flask contains 5.0 x 10 ^-2 mole of N2, 4.0 x 10^2 mg O2 , and 3.1 x 20^21 molecules of NH3. What is the partial pressure of each gas, and what is the total pressure in the flask?arrow_forward(b) A mixture of helium, hydrogen and carbon dioxide gases are at a pressure of 1200 torr in a 4 L closed container. There are a total of 24 moles of gas molecules in the container. If the helium concentration is 2 moles/L and hydrogen concentration is 1.5 moles/L, estimate the partial pressure of carbon dioxide in atm.arrow_forward
- The synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g) + 3 H2(g) → 2 NH3(g) Suppose that at one stage in the reaction, 13 mol NH3, 31 mol N2, and 93 mol H, are present in the reaction vessel at a total pressure of 210 atm. Calculate the mole fraction of NH3 and its partial pressure.arrow_forwardA gas mixture that has the following composition in percent by volume: 9.2% CO2, 22.0% CO, 17.5% H2, 3.3% CH4 and 48.0% N2. (a) What is the density of this gas at 22 o C and 755 mmHg, in grams per liter? (b) What is the partial pressure of CO2 in this mixture at 0.00 o C and 1 atm? (c) What volume of air is required for the complete combustion of this mixture of gas? (Air contains 20.9% O2 by volume)arrow_forwardConsider the following chemical reaction:C(s)+H2O(g)→CO(g)+H2(g) How many liters of hydrogen gas are formed from the complete reaction of 1.07 molmol of CC? Assume that the hydrogen gas is collected at a pressure of 1.0 atmatm and a temperature of 317 KK .arrow_forward
- consider an experiment where 4.55mL of an unknown H2O2(aq) solution reacted with the yeast at 19.1 C to produce 98.10ml of gas. what is the partial pressure of O2 (in atm) in the collected gas? 1.0126 atm O2 (this is the correct answer. Can you please show me how to get this calculation) How many moles of O2 were produced by the reaction? 0.004142 mol O2 is the answer.arrow_forwardA 4.0-liter rigid metal can is filled with nitrogen gas at 45 °C to a pressure of 1.125 atm. The can is then placed in a refrigerator until the temperature decreases to –10 °C. From a molecular standpoint, (i) explain why the pressure of the gas will change by being put in the refrigerator then (ii) calculate what the new pressure will be.arrow_forwardA steel cylinder contains 5.00 moles graphite (pure carbon) and 5.00 moles O2. The mixture is ignited and all the graphite reacts. Combustion produces a mixture of CO gas and CO2 gas. After the cylinder has cooled to its original temperature, it is found that the pressure of the cylinder has increased by 30.0 %. Calculate the mole fractions of CO, CO2, and O2 in the final gaseous mixture. Mole fraction of CO = Mole fraction of CO2 = Mole fraction of O2 =arrow_forward
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