Journal Entry:

Under which of the following sets of conditions is 1L of a gas equal to 1 mole of a gas?

(A) Pressure: 8.21 atm, Temperature: 10.00 K

(B) Pressure: 22.4 atm, Temperature: 273 K

(C) Pressure: 273 atm, Temperature: 8.21 K

(D) Pressure: 40.0 atm, Temperature: 300.0 K

Learning Intentions

• We will learn how to analyze data similar to lab to determine molar mass of an unknown substance.

• We will learn how to determine partial pressure of a gas collected in a tube over water.

• We will learn how to convert quantities calculated at one condition into equivalent quantities in new conditions. 

Closing Task:

You can analyze data similar to lab done in class to determine molar mass of an unknown.

You can compare predicted volume of hydrogen produce in reaction between magnesium and hydrochloric acid to actual volume of hydrogen using gas laws.

Content Standards being covered:

The gaseous state can be effectively modeled with a mathematical equation relating various macroscopic properties. A gas has neither a definite volume nor a definite shape, because the effects of attractive forces are minimal, we usually assume that the particles move independently. (E.K. 2.A.2)