For this equation, (NH4)2Cr2O7(s) ? Cr2O3(s) + N2(g) + 4H2O(g) , an engineer has to calculate the volume of gases that are produced under standard temperature and pressure conditions, given that 1,458 g of ammonium dichromate will decompose. Select the three values that they need to solve this problem. the molar mass of water The molar ratio from the balanced equation Avogadro's number: 6.02e23 particles/mol STP molar gas volume: 22.4 L/mol the molar mass of nitrogen gas the molar mass of ammonium dichromate
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First, we need to find the moles of ammonium dichromate that will decompose. For this, we need the molar mass of ammonium dichromate. Show more…
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Nitrogen gas is a product of the thermal decomposition of ammonium dichromate, (NH_), Cr,O_: $$\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(s) \rightarrow \mathrm{N}_{2}(g)+\mathrm{Cr}_{2} \mathrm{O}_{3}(s)+4 \mathrm{H}_{2} \mathrm{O}(g)$$ How many liters of $\mathrm{N}_{2}$ are produced during the decomposition of 100.0 grams of ammonium dichromate $(M=252.07 \mathrm{g} / \mathrm{mol})$ at $22^{\circ} \mathrm{C}$ and a pressure of 757 torr?
When heated by a flame, ammonium dichromate decomposes, producing nitrogen gas, solid chromium(III) oxide, and water vapor \begin{equation} \left(\mathrm{NH}_{4}\right) 2 \mathrm{Cr}_{2} \mathrm{O}_{7} \rightarrow \mathrm{N}_{2}+\mathrm{Cr}_{2} \mathrm{O}_{3}+4 \mathrm{H}_{2} \mathrm{O} \end{equation} Write the mole ratios for this reaction that relate ammonium dichromate to the products.
Nitrogen gas is a product of the thermal decomposition of ammonium dichromate, (NH4)2Cr2O7: (NH4)2Cr2O7(s) → N2(g) + Cr2O3(s) + 4 H2O(g). How many liters of N2 are produced during the decomposition of 100.0 grams of ammonium dichromate (M = 252.07 g/mol) at 22°C and a pressure of 757 torr?
David C.
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