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14 August, 02:29

2. When heated above 500 ºC, potassium nitrate decomposes according to the equation below. 4KNO3 2K2O + 2N2 + 5O2A. If oxygen is being formed at a rate of 0.30 M/s, what are the rates of formation of the other products? B. What is the rate at which the potassium nitrate is decomposed?

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  1. 14 August, 02:57
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    (a) The rate of formation of K2O is 0.12 M/s.

    The rate of formation of N2 is also 0.12 M/s

    (b) The rate of decomposition of KNO3 is 0.24 M/s

    Explanation:

    (a) From the equation of reaction, the mole ratio of K2O to O2 is 2:5.

    Rate of formation of O2 is 0.3 M/s

    Therefore, rate of formation of K2O = (2*0.3/5) = 0.12 M/s

    Also from the equation of reaction, mole ratio of N2 to O2 is 2:5.

    Rate of formation of N2 = (2*0.3/5) = 0.12 M/s

    (b) From the equation of reaction, mole ratio of KNO3 to O2 is 4:5.

    Therefore, rate of decomposition of KNO3 = (4*0.3/5) = 0.24 M/s
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