Question

All entries in the following table involve pressure-volume-temperature-amount data for a sample of a gas. Each row in the table is a separate set of data. Based on the ideal gas law, fill in the blank in each row in the table. The first row in the table is already completed as an example. P V n T 10.9 atm 3.00 L 1.00 mole 127°C a. 22.4 atm 3.00 mole 27°C b. 8.00 L 2.00 mole 73°C c. 2.50 atm 2.50 L -173°C d. 5.00 atm 10.0 L 2.00 mole

          All entries in the following table involve pressure-volume-temperature-amount data for a sample of a gas. Each row in the table is a separate set of data. Based on the ideal gas law, fill in the blank in each row in the table. The first row in the table is already completed as an example.

P V n T
10.9 atm 3.00 L 1.00 mole 127°C
a. 22.4 atm 3.00 mole 27°C
b. 8.00 L 2.00 mole 73°C
c. 2.50 atm 2.50 L -173°C
d. 5.00 atm 10.0 L 2.00 mole

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All entries in the following table involve pressure-volume-temperature-amount data for a sample of a gas. Each row in the table is a separate set of data. Based on the ideal gas law, fill in the blank in each row in the table. The first row in the table is already completed as an example.

P V n T
10.9 atm 3.00 L 1.00 mole 127°C
a. 22.4 atm 3.00 mole 27°C
b. 8.00 L 2.00 mole 73°C
c. 2.50 atm 2.50 L -173°C
d. 5.00 atm 10.0 L 2.00 mole

Added by Milagros C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Cheryl Glor

04/28/2023

Step 1

The ideal gas constant, R, can be given in different units, but since we have pressure in atm and volume in L, we will use R = 0.0821 L atm / (mol K). Now, let's fill in the blanks for each row: Row 1 (already completed): P = 10.9 atm V = 3.00 L n = 1.00 mole T Show more…

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All entries in the following table involve pressure-volume-temperature-amount data for a sample of a gas. Each row in the table is a separate set of data. Based on the ideal gas law, fill in the blank in each row in the table. The first row in the table is already completed as an example. P V n T 10.9 atm 3.00 L 1.00 mole 127°C a. 22.4 atm 3.00 mole 27°C b. 8.00 L 2.00 mole 73°C c. 2.50 atm 2.50 L -173°C d. 5.00 atm 10.0 L 2.00 mole

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Transcript

00:01 Here we have a table that we have to complete and we're going to be using pv equals nrt a bunch of different times.

00:08 So let's take a look at pivner and let's solve it for p.

00:12 Here p is going to equal n rt all over v.

00:19 Now let's take a look at volume.

00:21 If we're going to be solving it for volume, that's going to be nrt all over p.

00:28 Well that equals your volume.

00:30 Now the number of moles, that is pv over rt.

00:36 And scroll to give us a little more room.

00:39 And if we're solving it for your temperature, remember we have pv equals nrt.

00:46 Temperature is going to be pv over nr.

00:51 So this entire time i'm going to be using the r value of 0 .082057.

01:04 And the units are liters, atmospheres over mole kelvin.

01:10 So we were given everything in temperatures of degree c, so i went ahead and converted it to temperatures for kelvin.

01:17 And all i did was added 273 .15 to each one of our degrees celsius, so that got us two degrees kelvin.

01:28 So let's take a look at a where we have to solve for the volume.

01:36 So for solving for the volume we're going to have 3 times 0 .082057 times 300 .15 all over 22 .4.

01:51 So let's do this math.

01:53 3 times 0 .082057 times 300 .15, then divide that by 22 .4...

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