Question

From the balanced reaction below, when you have 3.33 moles of (NH4)2Cr2O7, how many grams of N2 will be produced

Answer 1

`m_(N_2)=93.3gN_2`

Step-by-step explanation:

Hello there!

In this case, for this stoichiometry-based problem, it is firstly necessary to realize that the decomposition of ammonium dichromate is given by:

`(NH_4)_2Cr_2O_7(s)\rightarrow N_2(g)+4H_2O(l)+Cr_2O_3(s)`

Thus, since the mole ratio between ammonium dichromate and the gaseous nitrogen (molar mass = 28.02 g/mol) is 1:1, we can compute the produced mass of the latter via stoichiometry as shown below:

`m_(N_2)=3.33mol(NH_4)_2Cr_2O_7*(1molN_2)/(1mol(NH_4)_2Cr_2O_7)*(28.01gN_2)/(1molN_2)\\\\ m_(N_2)=93.3gN_2`

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