Untitled Quiz

There are two main types of natural gas. Dry natural gas mainly contains methane. Wet natural gas includes methane, but also contains ethane, propane, butane and pentane.

Natural gas has various uses including domestic (heating, cooking), industrial production, power generation, vehicle fuel, fertilizer production, and hydrogen fuel cells.

Stoichiometry is the study of the relationships between amounts of substances involved in chemical reactions. It focuses on mass and volume relationships in unit operations and processes.

This principle states that a pure chemical substance always contains its elements in the same proportions by weight. It also states that when two elements combine to form different compounds, their weights are always in a simple ratio.

The application of the laws of conservation of matter, elements, and energy to industrial chemical processes and operations. It helps us understand the efficiency and effectiveness of chemical reactions in industry.

A chemical reaction involving a fuel reacting with oxygen (usually from air) to release energy in the form of heat. This process is important for heat generation in various industries.

Studying combustion is essential in chemical engineering, as it is a crucial step in many chemical processes where heat is needed. This field focuses on understanding and optimizing the combustion process.

Combustion is a common and essential industrial process used for heat generation. It involves the reaction between oxygen and a fuel source.

The simplest whole-number ratio of atoms of each element present in a compound.

Divide the mass of each element by its molar mass to find the number of moles present.

1. Find the moles of each element. 2. Divide each mole value by the smallest mole value. 3. Express the resulting ratios as the smallest whole numbers.

Mass of Oxygen = Total sample mass - Mass of Carbon - Mass of Hydrogen

A technique used to determine the empirical formula of a compound by burning it in oxygen and measuring the masses of CO2 and H2O produced.

1. React the compound with sodium to form a chloride salt. 2. Dissolve the salt and precipitate chloride ions using AgNO3.

The mass of AgCl produced is directly related to the mass of chlorine present in the original compound.

A separate analysis using a different method helps confirm the empirical formula found through combustion analysis.

The actual number of atoms of each element in a molecule of a compound.

The sum of the atomic weights of all the atoms in the empirical formula.

The ratio of the molecular weight (MW) to the empirical weight (EW).

1. Find the moles of each element.
2. Divide each mole value by the smallest mole value to obtain a ratio.
3. If necessary, multiply the ratios by a whole number to get whole numbers.
4. Write the empirical formula using the whole number ratios as subscripts.

1. Calculate the empirical weight (EW).
2. Divide the molecular weight (MW) by the empirical weight (EW) to get the formula weight ratio (R).
3. Multiply the ratio (R) by the subscripts in the empirical formula to get the molecular formula.

The empirical formula shows the simplest whole-number ratio of atoms in a compound, while the molecular formula shows the actual number of atoms of each element in a molecule.

The empirical formula gives us the simplest ratio of atoms in a compound, but it doesn't tell us the actual number of atoms in a molecule. To determine the actual number of atoms, we need to find the molecular formula.

To find the amount of carbon in a sample, use the mass of carbon dioxide (CO2) produced and the molar mass of carbon and CO2. Divide the mass of CO2 by its molar mass (44 g/mol), then multiply by the ratio of the molar mass of carbon (12 g/mol) to the molar mass of CO2.

To find the amount of hydrogen in a sample, use the mass of water (H2O) produced and the molar masses of hydrogen and water. Divide the mass of water by its molar mass (18 g/mol), then multiply by the ratio of twice the molar mass of hydrogen (2 g/mol) to the molar mass of water.

To find the amount of chlorine in a sample, use the mass of silver chloride (AgCl) produced and the molar masses of chlorine and AgCl. Divide the mass of AgCl by its molar mass (143.32 g/mol), then multiply by the ratio of the molar mass of chlorine (35.45 g/mol) to the molar mass of AgCl.

To find the amount of chlorine in a sample when given the mass of a second sample and the amount of chlorine in that sample, apply the principle of ratio and proportion. Set up a proportion: the ratio of the mass of chlorine to the mass of the first sample equals the ratio of the mass of chlorine to the mass of the second sample. Solve for the unknown mass of chlorine in the first sample.

The calculations are performed to determine the elemental composition of the samples. This information is crucial for understanding the chemical formula of the unknown compound(s) present in the samples.

The calculated amounts of each element are used to determine the empirical formula of the unknown compound. The empirical formula represents the simplest whole-number ratio of atoms in the compound.

The mass of an element within a sample is directly proportional to the sample's overall mass. This means that changing the sample size will proportionally change the amount of each element present.

A method used to analyze the composition of flue gases, excluding water vapor (H2O) and sulfur trioxide (SO3).

The chemical reaction where formaldehyde reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).

The amount of oxygen supplied beyond what is theoretically required for complete combustion of a fuel.

The ideal amount of oxygen needed for complete combustion of a fuel, based on stoichiometry.

The percentage of oxygen supplied in excess of the theoretical requirement.

The composition of gases released from a combustion process, typically including CO2, N2, O2, and H2O.

Describes a flue gas composition where all of the available oxygen has been consumed during combustion.

Nitrogen is a major component of flue gas, originating from the air supplied during combustion.

The gas produced by burning a fuel, usually containing carbon dioxide (CO2), nitrogen (N2), and sometimes oxygen (O2).

Orsat analysis is used to determine the composition of gases, particularly flue gas, to understand the efficiency of combustion and potential for pollutant emissions.

CO2 is produced during complete combustion of carbon-containing fuels, where all the carbon in the fuel combines with oxygen.

'O2-free' in an Orsat analysis indicates the volume of oxygen that has been consumed during the combustion process.

Carbon monoxide (CO) is produced during incomplete combustion, where not all the carbon in the fuel has combined with oxygen.

Water is produced when hydrogen (H) in the fuel combines with oxygen (O) during combustion.

Method II is more appropriate for this problem because it directly accounts for the specific fuel being burned, unlike Method I which relies on theoretical values.

The oxygen supplied is greater than the oxygen consumed because some oxygen is leftover after combustion, while some is used for other reactions.

The amount of nitrogen in the air supplied is needed to calculate the complete composition of the flue gas, ensuring a balanced chemical equation.