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Chapter 8: Q. 8.41 (page 273)

Rearrange the variable in the combined gas law to solve for $T_{2}$ .

Short Answer

Expert verified

The combined gas law for $T_{2}$ is role="math" localid="1652612034505" $T_{2} = \frac{T_{1} \times P_{2} \times V_{2}}{P_{1} \times V_{1}}$ .

Step by step solution

01

Given Information

We need to rearrange the variable in combined gas law to solve for $T_{2}$

02

Simplify

The combined gas law is given as:

$\frac{P_{1} \times V_{1}}{T_{1}} = \frac{P_{2} \times V_{2}}{T_{2}}$

Here,

$P_{1}$ is initial pressure,

$T_{2}$ is initial temperature,

role="math" localid="1652611570206" $V_{1}$ is initial volume,

$P_{2}$ is final pressure,

role="math" localid="1652611612307" $T_{2}$ is final temperature and

$V_{2}$ is the final volume.

Now, in case if are asked to find the final temperature the combined gas equation will be rearranged as:

$\frac{P_{1} \times V_{1}}{T_{1}} = \frac{P_{2} \times V_{2}}{T_{2}} T_{2} \times P_{1} \times V_{1} = T_{1} \times P_{2} \times V_{2}$

For $T_{2}$ is equal to:

$T_{2} = \frac{T_{1} \times P_{2} \times V_{2}}{P_{1} \times V_{1}}$

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Most popular questions from this chapter

A head injury can affect the ability of a person to ventilate(breath in and out).

a. What would happen to the partial pressure of oxygen and carbon dioxide in the blood if a person cannot properly ventilate?

b. When a person who cannot breathe properly is placed on a ventilator, an air mixture is delivered at pressures that are alternately above the air pressure in the person's lung, and then below. How will this move oxygen into the lungs, and carbon dioxide out?

Indicate if pressure increase decreases, or stays the same in each of the following: $(8.2, 8.4, 8.6)$

A scuba diver $60 f t$ below the ocean surface inhales $50.0 m L$ of compressed air from a ccuba tank at a pressure of $3.00 a t m$ and a temperature of $8 ° C$ . What is the final pressure of air, in atmospheres, in the lungs when the gas expands to $150.0 m L$ at a body temperature of $37 ° C$ , if the amount of gas does not change?

Two flasks of equal volume and at the same temperature contain different gases. One flask contains $5.0 g o f H_{2}$ . Is each of the following statements true or false? Explain. $(8.1)$

a. Both flasks contain the same number of molecules.

b. The pressure in the the flasks are the same.

A sample of Ne gas has a pressure of 654 mmHg with an unknown volume. The gas has a pressure of 345 mmHg when the volume is 495 mL, with no change in temperature or amount of gas. What was the initial volume, in milliliters, of the gas?

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