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Question: For the reaction \(4NH_{3} + 5O_{2} \rightarrow 4NO + 6H_{2}O,\) if the rate of disappearance of \(N...

For the reaction 4NH3+5O2→4NO+6H2O,4NH_{3} + 5O_{2} \rightarrow 4NO + 6H_{2}O, if the rate of disappearance of NH3NH_{3} is 3.6×10−3molL−1s−13.6 \times 10^{- 3}molL^{- 1}s^{- 1} what is the rate of formation of H2OH_{2}O?

A

5.4×10−3molL−1s−15.4 \times 10^{- 3}molL^{- 1}s^{- 1}

B

3.6×10−3molL−1s−13.6 \times 10^{- 3}molL^{- 1}s^{- 1}

C

4×10−4molL−1s−14 \times 10^{- 4}molL^{- 1}s^{- 1}

D

0.6×10−4molL−1s−10.6 \times 10^{- 4}molL^{- 1}s^{- 1}

Answer

5.4×10−3molL−1s−15.4 \times 10^{- 3}molL^{- 1}s^{- 1}

Explanation

Solution

−14d[NH3]dt=+16d[H2O]dt- \frac{1}{4}\frac{d\lbrack NH_{3}\rbrack}{dt} = + \frac{1}{6}\frac{d\lbrack H_{2}O\rbrack}{dt}

d[H2O]dt=64×3.6×10−3=5.4×10−3molL−1s−1\frac{d\lbrack H_{2}O\rbrack}{dt} = \frac{6}{4} \times 3.6 \times 10^{- 3} = 5.4 \times 10^{- 3}molL^{- 1}s^{- 1}