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- Homework Statement:
- Integrated rate law calculations
- Relevant Equations:
The decomposition of ammonia on a platinum surface at 856 °C
NH31/2 N2 + 3/2 H2
is zero order in NH3 with a rate constant of 1.50×10-6M s-1.
If the initial concentration of NH3 is 5.28×10-3 M, the concentration of NH3 will be ___
M after 2.54×103seconds have passed.
The decomposition of nitrosyl bromide at 10 °C
NOBrNO + ½ Br2
is second order in NOBr.
In one experiment, when the initial concentration of NOBr was 0.341 M, the concentration of NOBr dropped to 7.81×10-2 M after 9.06seconds had passed.
Based on these data, the rate constant for the reaction is ___
The gas phase decomposition of nitrogen dioxide at 383 °C
NO2(g)NO(g) + ½ O2(g)
is second order in NO2 with a rate constant of 0.540M-1 s-1.
If the initial concentration of NO2 is 0.131 M, the concentration of NO2 will be 3.28×10-2 M after
___ seconds have passed.
No idea how to solve