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

Question

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

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Delwyn 5 months 2021-09-04T16:32:36+00:00 1 Answers 9 views 0

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    2021-09-04T16:34:14+00:00

    Answer:

    m_{N_2}=93.3gN_2

    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*\frac{1molN_2}{1mol(NH_4)_2Cr_2O_7}*\frac{28.01gN_2}{1molN_2}\\\\  m_{N_2}=93.3gN_2

    Best regards!

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