Question

Determine the number of moles of gas contained in each of the following: a. 1.25 L at 250.0 K and 1.06 atm b. 0.80 L at 27°C and 0.925 atm c. $7.50 \times 10^{2} mL$ at $-50.0^{\circ} C$ and 0.921 $atm$

Name: Problem 51, Chapter 11: Holt: Modern Chemistry
Uploaded: 2020-10-08T21:00:42-08:00
Duration: 1 min 49 s
Channel: David Collins
Description: Determine the number of moles of gas contained in each of the following: a. 1.25 L at 250.0 K and 1.06 atm b. 0.80 L at 27°C and 0.925 atm c. 7.50 ×10^2 mL at -50.0^∘ C and 0.921 atm

   Determine the number of moles of gas contained in each of the following:

a. 1.25 L at 250.0 K and 1.06 atm
b. 0.80 L at 27°C and 0.925 atm
c. $7.50 \times 10^{2} mL$ at $-50.0^{\circ} C$ and 0.921 $atm$

Holt: Modern Chemistry

Mickey Sarquis,… 1st Edition

Chapter 11, Problem 51

Instant Answer

Solved by Expert David Collins

10/08/2020

Step 1

We can rearrange this equation to solve for n, the number of moles, which gives us n = PV/RT. Show more…

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Determine the number of moles of gas contained in each of the following: a. 1.25 L at 250.0 K and 1.06 atm b. 0.80 L at 27°C and 0.925 atm c. $7.50 \times 10^{2} mL$ at $-50.0^{\circ} C$ and 0.921 $atm$

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Key Concepts

Volume Unit Conversion

Volume values must be in proper units (liters) when used in the ideal gas law. Converting between milliliters and liters is necessary, as 1000 mL equals 1 L, ensuring consistency in units across the formula.

Ideal Gas Law

This principle relates pressure, volume, moles of gas, and temperature via the equation PV = nRT. It is fundamental in determining the number of moles present in a given sample under specified conditions using a constant (R) that provides the relation between these properties.

Temperature Conversion

Since the ideal gas law requires temperature to be in Kelvin, converting from degrees Celsius to Kelvin is essential. This process involves adding 273.15 to the Celsius temperature, ensuring that the temperature is in the correct unit for calculations.

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