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Problem: A miniature volcano can be made in the laboratory with ammonium dichromate. When ignited, it decomposes in a fiery display. (NH4)2Cr2O7 (s) → N2 (g) + 4H2O (g) + Cr2O3 (s) If 0.76 g of ammonium dichromate is used, and the gases from this reaction are trapped in a 15.1 L flask at 29°C, what is the total pressure of the gas in the flask? What are the partial pressures of N2 and H2O? 

🤓 Based on our data, we think this question is relevant for Professor Parkin's class at COLUMBIA.

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A miniature volcano can be made in the laboratory with ammonium dichromate. When ignited, it decomposes in a fiery display. 

(NH4)2Cr2O7 (s) → N(g) + 4H2O (g) + Cr2O3 (s) 

If 0.76 g of ammonium dichromate is used, and the gases from this reaction are trapped in a 15.1 L flask at 29°C, what is the total pressure of the gas in the flask? What are the partial pressures of N2 and H2O? 

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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. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

What professor is this problem relevant for?

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