Based on the ideal gas law, there is a simple equivalency that exists between the amount of gas and the volume it occupies. At standard temperature and pressure (STP; 273.15 K and 1 atm, respectively), one mole of gas occupies 22.4 L of volume.
What mass of methanol (CH3OH) could you form if you reacted 5.39 L of a gas mixture (at STP) that contains an equal number of carbon monoxide (CO) and hydrogen gas (H2) molecules?
Express the mass in grams to three significant digits.
Carbon monoxide (CO) can react with hydrogen gas (H2) to form methanol (CH3OH) as shown in the Carbon Monoxide and Hydrogen - Sample 2 reaction in the simulation. The same reactants can also form methane (CH4) and water (H2O) as shown in the Carbon Monoxide and Hydrogen - Sample 1 reaction in the simulation. The latter reaction (Sample 1) is actually more commonly employed in reverse as a method for producing hydrogen gas, a process known as steam reforming, but it requires a lot of heat.
For the following exercises, you can track and confirm the amounts of reactants and products (in both moles and mass) using the Run Experiment tool under the Experiment tab in the simulation. Note that the simulation checks your values to a different number of significant digits than this tutorial. We will explore these two reactions of carbon monoxide and hydrogen.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.