Ammonium dichromate decomposes according to the following equation: (NH4)2Cr2O7(

Question

Ammonium dichromate decomposes according to the following equation: (NH4)2Cr2O7(s) -> N2(g) + 4H2O(g) + Cr2O3(s)

Part 1) If 0.95 g of ammonium dichromate is used, and if the gases from this reaction are trapped in a 15.0 L flask at 23 deg. C. How many moles of N2 and H2O are produced from (9.42x10^-1) g of (NH4)2Cr2O7 (MW = 252 g/mol)?

Part 2) How much pressure is caused by (1.78x10^-2) mol of N2 and H2O if the gases from this reaction are trapped in a 15.0 L flask at 27 deg. C? The correct answer has 3 SF's and remember to specify the unit by its symbol

Part 3) How many moles of H2O are produced from (1.68x10^-2) mol of (NH4)2Cr2O7?

Explanation / Answer

part 1) (NH4)2Cr2O7(s) -> N2(g) + 4H2O(g) + Cr2O3(s)

n of (NH4)2Cr2O7(s)  -> n of  N2(g) +4n of 4H2O(g)

n of (NH4)2Cr2O7(s) = w/mw =0.95/252 = 0.003 moles

n of  N2(g)=0.003 moles

4n of 4H2O=0.003 moles*4

part 3) (1.68x10^-2) *4

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