(I pt.) Explain the difference between a real gas and an ideal gas. (Begin by de
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(I pt.) Explain the difference between a real gas and an ideal gas. (Begin by defining both terms and then explain how they are different.) Under what conditions does a real gas assume ideal gas behavior? 1. Show all calculations with units in your setups and the final answer for the following. (1 pt.) A sample of nitrogen was collected over water at a temperature of 30.0 °C. If the total pressure of the (wet) gas sample was 745 torr, what was the pressure of the nitrogen gas alone? The vapor pressure of water vapor at 30.0 °C-31.8 mm Hg. 2. 3. (2 pts.) A sample of 0.0430 g magnesium reacts with excess hydrochloric acid according to the following equation: The hydrogen gas is collected over water at 22 C and a pressure of 749.2 mm Hg. The volume of hydrogen gas collected was 43.2 mL. The barometric pressure is recorded as 749.2 mm of Hg. The vapor pressure of water vapor at 22 °C = 19.8 mm Hg. Calculate the percent purity of magnesium in the sample.Explanation / Answer
Question 1
Ideal gas is a hypothetical gas which obeys all the gas laws exactly. Ideal gas have no spaces between its molecules and have no molecular interactions in between
On the other hand real gas adhere to gas laws. These gases are practical as the molecules have space between them and they have intermolecular forces.
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