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Chapter 8: Problem 124

At STP, \(1.0 \mathrm{L}\) \(Br\) \(_{2}\) reacts completely with \(3.0 \mathrm{L} \mathrm{F}_{2}\), producing \(2.0 \mathrm{L}\) of a product. What is the formula of the product? (All substances are gases.)

Short Answer

Expert verified
The formula of the product produced when 1.0 L Br₂ reacts completely with 3.0 L F₂ at STP is BrF₃.

Step by step solution

01

Identify the given information and write down the balanced equation

First, let's identify the given information: - 1.0 L of Br₂ reacts completely - 3.0 L of F₂ are also reacting - 2.0 L of a product is produced The balanced equation is currently unknown, so we'll represent it as follows: Br₂(g) + F₂(g) ⟶ Product(g)
02

Use Avogadro's law

According to Avogadro's law, at the same temperature and pressure, equal volumes of different gases contain an equal number of molecules (or moles). Therefore, we can determine the mole ratios of the reactants and the product based on the given volumes. From the given information, we know: - 1.0 L Br₂ = 1 mole Br₂ - 3.0 L F₂ = 3 moles F₂ - 2.0 L Product = 2 moles Product
03

Determine the mole ratio of the reactants and product

Now that we have the moles of the reactants and product, we can determine their ratios. For Br₂ and F₂, we notice that the ratio of Br₂ to F₂ is 1:3 (1 mole Br₂: 3 moles F₂), and the product ratio is 2 moles. To find the complete ratio of the reactants to the product, let's use a bit of intuition. We know that Br₂ and F₂ are diatomic (Br₂ & F₂). Since Br₂ is interacting with three times more F₂, it is logical to deduce that each Br might form a bond with three F atoms. Thus, we can propose a probable product - BrF₃.
04

Revise the original balanced equation and confirm the mole ratios

With the probable formula of the product, we can now revise the original balanced equation: Br₂(g) + 3F₂(g) ⟶ 2BrF₃(g) Now, let's confirm the mole ratios with this equation: - 1 mol Br₂ : 3 mol F₂ - Producing 2 mol of BrF₃ The revised balanced equation is consistent with the given information in terms of both reactant ratios and product volume. Hence, we can conclude:
05

Answer the question

The formula of the product produced when 1.0 L Br₂ reacts completely with 3.0 L F₂ at STP is BrF₃.

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Most popular questions from this chapter

A gas sample containing \(1.50\) moles at \(25^{\circ} \mathrm{C}\) exerts a pressure of \(400 .\) torr. Some gas is added to the same container and the temperature is increased to \(50 .^{\circ} \mathrm{C}\). If the pressure increases to \(800 .\) torr, how many moles of gas were added to the container? Assume a constant-volume container.

A \(20.0\) -\(\mathrm{L}\) stainless steel container at \(25^{\circ} \mathrm{C}\) was charged with \(2.00\) atm of hydrogen gas and \(3.00\) atm of oxygen gas. A spark ignited the mixture, producing water. What is the pressure in the tank at \(25^{\circ} \mathrm{C} ?\) If the exact same experiment were performed, but the temperature was \(125^{\circ} \mathrm{C}\) instead of \(25^{\circ} \mathrm{C},\) what would be the pressure in the tank?

A steel cylinder contains \(5.00\) moles of graphite (pure carbon) and \(5.00\) moles of \(\mathrm{O}_{2}\). The mixture is ignited and all the graphite reacts. Combustion produces a mixture of \(\mathrm{CO}\) gas and \(\mathrm{CO}_{2}\) gas. After the cylinder has cooled to its original temperature, it is found that the pressure of the cylinder has increased by \(17.0 \% .\) Calculate the mole fractions of \(\mathrm{CO}, \mathrm{CO}_{2},\) and \(\mathrm{O}_{2}\) in the final gaseous mixture.

Ideal gas particles are assumed to be volumeless and to neither attract nor repel each other. Why are these assumptions crucial to the validity of Dalton's law of partial pressures?

Trace organic compounds in the atmosphere are first concentrated and then measured by gas chromatography. In the concentration step, several liters of air are pumped through a tube containing a porous substance that traps organic compounds. The tube is then connected to a gas chromatograph and heated to release the trapped compounds. The organic compounds are separated in the column and the amounts are measured. In an analysis for benzene and toluene in air, a \(3.00-\mathrm{L}\) sample of air at \(748\) torr and \(23^{\circ} \mathrm{C}\) was passed through the trap. The gas chromatography analysis showed that this air sample contained \(89.6\) ng benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) and \(153 \mathrm{ng}\) toluene \(\left(\mathrm{C}_{7} \mathrm{H}_{8}\right) .\) Calculate the mixing ratio (see Exercise 121 ) and number of molecules per cubic centimeter for both benzene and toluene.
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