Write a balanced equation for the monochlorination of butane c4h10

Need help with a chemistry question? Balancing equations is not my strong suit. I just need to pass this class and put chemistry behind me. One of the questions I am stuck on is this:

Write a balanced equation for the monochlorination of butane c4h10

This, in turn, allows us to easily handle such problems as the following: Is this answer reasonable? Yes, because the mass of CO must always be smaller than that of CO2 in this reaction. Mastering mass-mass problems Don't expect to pass Chemistry unless you can handle problems such as the ones below; they come up frequently in all kinds of contexts.

If you feel the need for more guidance, see one of the video tutorials listed near the bottom of this page. Assuming that the conversion is complete, how many liters of sulfuric acid density 1.

As with most problems, this breaks down into several simpler ones.

Key Concepts

The molar masses of the two components are Yes, because density tells us that the number of liters of acid will be slightly greater than half of its weight.

This water can be driven off by heat; if 1. What is the value of x in the formula of the hydrate? The first step is to find the number of moles of BaCl2 molecular weight This means that one or more reactant will usually be present in excess; there will be more present than can react, and some will remain after the reaction is over.

At the same time, one reactant will be completely used up; we call this the limiting reactant because the amount of this substance present will control, or limit, the quantities of the other reactants that are consumed as well as the amounts of products produced.

Limiting reactant problems are handled in the same way as ordinary stoichiometry problems with one additional preliminary step: If this comes to less than 0. If the limiting reactant is A, then all 0. How many grams of Cu2S can be made from 10 g of sulfur and 15 g of copper?

From the atomic weights of Cu Yes, because the chemical factor Air-to-fuel ratios in combustion Combustion is an exothermic process in which a fuel is combined with oxygen; complete combustion of a hydrocarbon fuel such as methane or gasoline yields carbon dioxide and water: Complete combustion of each kg of methane consumes 4 kg of dioxygen, which is supplied by the air.

In the classic Bunsen burner, this air is admitted through an adjustable opening near the base. When it is fully open, the flame is blue in color and achieves its maximum temperature, indicating that combustion is approximately stoichiometric. If the opening is gradually closed, the appearance of the flame changes as illustrated.

Under these conditions, oxygen becomes the limiting reactant and combustion is incomplete. Incomplete combustion is generally undesirable because it wastes fuel, produces less heat, and releases pollutants such as carbon soot.

Energy-producing combustion processes should always operate in fuel-limited mode. In ordinary combustion processes, the source of oxygen is air. Because only about 20 percent of the molecules in dry air consist of O2, the volume of air that must be supplied is five times greater than what would be required for pure O2.

For the detailed calculation, see here. In order to ensure complete combustion, it is common practice to maintain a slightly lean mixture. However, practical considerations necessitate differing ratios at various stages of operation.

Typical values vary from a rich ratio for starting or acceleration to slightly lean ratios for ordinary driving. These ratios are set by the carburetorwith additional control by the engine computer and exhaust-line oxygen sensor in modern vehicles, or by a manual choke in earlier ones.

write a balanced equation for the monochlorination of butane c4h10

Aerobic and anaerobic respiration Our bodies require a continual supply of energy in order to maintain neural activity, synthesize proteins and other essential biochemical components, replace cells, and to power muscular action. The "fuel" — the carrier of chemical energy — glucose, a simple sugar which is released as needed from the starch-like polymer glycogenthe form in which the energy we derive from food is stored.

Arterial blood carries dissolved glucose along with hemoglobin-bound dioxygen to individual cells which are the sites of glucose "combustion": Because this process utilizes oxygen from the air we breath, it is known as aerobic respiration. And as with any efficient combustion process, glucose is the limiting reactant here.

But there are times when vigorous physical activity causes muscles to consume glucose at a rate that exceeds the capacity of the blood to deliver the required quantity of oxygen.ORGANIC CHEM I Practice Questions for Ch. 4 1) Write an equation to describe the initiation step in the chlorination of methane.

2) Reaction intermediates that have unpaired electrons are called _____. 3) When light is shined on a mixture of chlorine and chloromethane, methylene chloride (dichloromethane) is one of the products. Our goal is to use a thermochemical equation to calculate the heat produced when a specific amount of methane gas is combusted.

According to Equation , kJ is released by the system when 1 mol CH. 4. is burned at constant pressure (Δ. H = – kJ).

Plan: Equation provides us with a stoichiometric conversion factor: 1 mol CH. 4 – kJ).

Example 1 Molecular and Empirical Formulas

Jun 27,  · Butane, C4H10 is a fuel used in lighters. When butane burns, it combines with oxygen to produce carbon dioxide and water. A student burned a gram sample of butane.

A.) Write a balanced equation for the combustion of butane B.) Find the number of grams of carbon dioxide produced from g butaneStatus: Resolved. How do I balance this combustion reaction?

Ask Question 4 Balanced equation for the combustion of $\ce{C4H8}$ is $$\ce{C4H8 + 6O2 -> 4CO2 + 4H2O}$$ Nitrogen is included only to indicate that it is present in the medium with some specific ratio to the oxygen amount --well technically it is included to make question look complicated. + Cl2 + HCl Cl Write a balanced equation for each reaction: A) complete combustion of cyclobutane B) monobromination of propane C) complete combustion of ethane D) monochlorination of butane Write a balanced equation for each reaction: A) complete combustion of cyclobutane 2 C4H10 + 13 O2 8 CO2 + 10 H2O + heat energy B) monobromination of.

6. Write a balanced equation describing each of the following chemical reactions. (a) Solid potassium chlorate, KClO3, decomposes to form solid potassium chloride and diatomic oxygen gas.

A. KClO3 (s) KCl (s) + O2 (g) (b) Solid aluminum metal reacts with solid diatomic iodine to form solid Al2I6.

Writing and Balancing Chemical Equations