Problem: Hydrogen cyanide is prepared commercially by the reaction of methane, CH4(g), ammonia, NH3(g), and oxygen, O2(g), at high temperature. The other product is gaseous water.b. What volume of HCN(g) can be obtained from the reaction of 20.0 L CH4(g), 20.0 L NH3(g), and 20.0 L O2(g)? The volumes of all gases are measured at the same temperature and pressure.

FREE Expert Solution

We are being asked to determine the volume of HCN(g) that can be obtained from the reaction of 20.0 L CH4(g), 20.0 L NH3(g), and 20.0 L O2(g)


We are going to do the following steps:

Step 1: Write the balanced equation

Step 2: Determine moles of each reactant

Step 3: Determine the limiting reactant

Step 4: Determine Liters of HCN


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Problem Details

Hydrogen cyanide is prepared commercially by the reaction of methane, CH4(g), ammonia, NH3(g), and oxygen, O2(g), at high temperature. The other product is gaseous water.
b. What volume of HCN(g) can be obtained from the reaction of 20.0 L CH4(g), 20.0 L NH3(g), and 20.0 L O2(g)? The volumes of all gases are measured at the same temperature and pressure.

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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 Gas Stoichiometry concept. You can view video lessons to learn Gas Stoichiometry. Or if you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

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Based on our data, we think this problem is relevant for Professor Forconi's class at COFC.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.