Administratium bromide (AdBr) decomposes readily at temperatures exceeding 37°C. The figure below shows how the rate of reaction varies with the concentration of AdBr. The rate, r, is in units of M s-1 and the concentration of AdBr, c, is in units of M (mole L-1). The slope has a value of a 1.67 and the intercept has a value of 0.490.
(a) What is the order of reaction?
(b) Calculate the instant rate of decomposition of AdBr when its concentration is 0.03091 M. Express your answer in M s-1.
Noted.
a--rate=k(AdBr)^r
ln (rate)=r ln ((AdBr)+ln k
r=1.67
ln k=0.490=>k=1.63
order of reaction=1.63
b-- and rate of decomposition r-1.63*(.03091)^1.67
=4.91*10^-3 m/s
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To determine the order of reaction, we need to analyze the relationship between the rate of reaction (r) and the concentration of AdBr (c) as shown in the figure. The given information about the slope and intercept can be used to find the order.
(a) The order of reaction can be determined by looking at the exponent of the concentration term in the rate equation. Since the slope of the graph represents the value of the exponent, we can conclude that the order of reaction is 1.67 (approximately).
(b) Now that we know the order of reaction is 1.67, we can use this information to calculate the instant rate of decomposition of AdBr when its concentration is 0.03091 M.
The rate equation for a first-order reaction can be written as: r = k * [AdBr]^n
Where:
- r is the rate of reaction
- k is the rate constant
- [AdBr] is the concentration of AdBr
- n is the order of reaction
Substituting the given values:
- n = 1.67 (order of reaction)
- [AdBr] = 0.03091 M (concentration of AdBr)
- k is the rate constant (unknown)
The rate equation becomes: r = k * (0.03091)^1.67
To find the value of k, we need additional information or experimental data.