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Chapter 5: Problem 26

Molecular chlorine and molecular fluorine combine to form a gaseous product. Under the same conditions of temperature and pressure it is found that one volume of \(\mathrm{Cl}_{2}\) reacts with three volumes of \(\mathrm{F}_{2}\) to yield two volumes of the product. What is the formula of the product?

Short Answer

Expert verified
The formula of the product is \(\mathrm{ClF}_{3}\).

Step by step solution

01

Identify the ratio of reacting volumes

The problem gives the ratio of the volumes of \(\mathrm{Cl}_{2}\), \(\mathrm{F}_{2}\), and the product as 1:3:2 respectively, according to their reaction.
02

Write unbalanced chemical reaction

Next is to write the chemical reaction using the known reactants, which are \(\mathrm{Cl}_{2}\) and \(\mathrm{F}_{2}\), and unknown product X. This forms: \(\mathrm{Cl}_{2} + \mathrm{F}_{2} \rightarrow X\)
03

Balance the chemical equation according to the gas volume ratio

Given the volume ratios are also the stoichiometric coefficients, the unknown product must contain 2 atoms of chlorine and 6 atoms of fluorine. Therefore, the balanced equation and hence the product becomes: \( \mathrm{Cl}_{2} + 3\mathrm{F}_{2} \rightarrow 2\mathrm{ClF}_{3}\)

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Most popular questions from this chapter

Lithium hydride reacts with water as follows: $$\mathrm{LiH}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{LiOH}(a q)+\mathrm{H}_{2}(g)$$ During World War II, U.S. pilots carried LiH tablets. In the event of a crash landing at sea, the LiH would react with the seawater and fill their life belts and lifeboats with hydrogen gas. How many grams of LiH are needed to fill a \(4,1-\mathrm{L}\) life belt at \(0.97 \mathrm{~atm}\) and \(12^{\circ} \mathrm{C} ?\)

A \(2.5-\mathrm{L}\) flask at \(15^{\circ} \mathrm{C}\) contains a mixture of three gases, \(\mathrm{N}_{2},\) He, and \(\mathrm{Ne},\) at partial pressures of \(0.32 \mathrm{~atm}\) for \(\mathrm{N}_{2}, 0.15 \mathrm{~atm}\) for \(\mathrm{He},\) and \(0.42 \mathrm{~atm}\) for Ne. (a) Calculate the total pressure of the mixture. (b) Calculate the volume in liters at STP occupied by He and Ne if the \(\mathrm{N}_{2}\) is removed selectively.

A sample of nitrogen gas kept in a container of volume \(2.3 \mathrm{~L}\) and at a temperature of \(32^{\circ} \mathrm{C}\) exerts a pressure of \(4.7 \mathrm{~atm} .\) Calculate the number of moles of gas present.

The apparatus shown in the diagram can be used to measure atomic and molecular speed. Suppose that a beam of metal atoms is directed at a rotating cylinder in a vacuum. A small opening in the cylinder allows the atoms to strike a target area. Because the cylinder is rotating, atoms traveling at different speeds will strike the target at different positions. In time, a layer of the metal will deposit on the target area, and the variation in its thickness is found to correspond to Maxwell's speed distribution. In one experiment it is found that at \(850^{\circ} \mathrm{C}\) some bismuth (Bi) atoms struck the target at a point \(2.80 \mathrm{~cm}\) from the spot directly opposite the slit. The diameter of the cylinder is \(15.0 \mathrm{~cm}\) and it is rotating at 130 revolutions per second. (a) Calculate the speed \((\mathrm{m} / \mathrm{s})\) at which the target is moving. (Hint: The circumference of a circle is given by \(2 \pi r\), in which \(r\) is the radius.) (b) Calculate the time (in seconds) it takes for the target to travel \(2.80 \mathrm{~cm} .\) (c) Determine the speed of the Bi atoms. Compare your result in (c) with the \(u_{\mathrm{rms}}\) of Bi at \(850^{\circ} \mathrm{C}\). Comment on the difference.

The temperature of \(2.5 \mathrm{~L}\) of a gas initially at STP is increased to \(250^{\circ} \mathrm{C}\) at constant volume. Calculate the final pressure of the gas in atm.
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