Structure 1.5—Ideal gases：練習問題

Which statement is a valid assumption of the kinetic molecular theory for an ideal gas?

A container holds $$2.0 \text{ mol}$$ of nitrogen gas and $$3.0 \text{ mol}$$ of oxygen gas at a total pressure of $$5.0 \text{ atm}$$. What is the partial pressure of nitrogen gas?

When $$10.0 \text{ g}$$ of calcium carbonate ($$CaCO_3$$) reacts completely with excess hydrochloric acid ($$HCl$$), what volume of carbon dioxide gas ($$CO_2$$) is produced at standard temperature and pressure (STP)?

The balanced chemical equation is:
$$CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + H_2O(l) + CO_2(g)$$

Which statement best describes an assumption of the ideal gas model?

A gas sample has a mass of $$2.50 \text{ g}$$ and occupies a volume of $$1.00 \text{ L}$$ at a pressure of $$1.20 \text{ atm}$$ and a temperature of $$25.0 \text{ °C}$$. What is the molar mass of the gas?

What is the molar volume of an ideal gas at Standard Temperature and Pressure (STP)?

Explain why real gases deviate from ideal gas behaviour at very low temperatures.

An ideal gas occupies $$2.5 \text{ L}$$ at $$300 \text{ K}$$ and $$1.0 \text{ atm}$$. If the temperature is increased to $$600 \text{ K}$$ and the volume is simultaneously reduced to $$1.25 \text{ L}$$, what will be the new pressure?

A sealed container of volume $$12.0 \text{ L}$$ holds a sample of nitrogen gas. The gas is at a temperature of $$30.0 \text{ °C}$$ and exerts a pressure of $$2.50 \text{ atm}$$.

Calculate the number of moles of nitrogen gas present in the container. (Gas constant R = $$0.0821 \text{ L atm mol}^{-1} \text{ K}^{-1}$$)

A sample of oxygen gas has a volume of $$15.0 \text{ L}$$ at a pressure of $$1.50 \text{ atm}$$ and a temperature of $$25.0 \text{ °C}$$.

a) Calculate the number of moles of oxygen gas in the sample.

b) If the temperature is increased to $$50.0 \text{ °C}$$ and the pressure is decreased to $$1.00 \text{ atm}$$, what will be the new volume of the oxygen gas, assuming the number of moles remains constant?