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3 years ago

6

What is the particle's position at t =3.0s ? express your answer to three significant figures and include the appropriate units?

1 answer:

Tcecarenko [31]3 years ago

8 0

The only given information is the time in 3 seconds. We are asked to find the position, or the distance traveled. The working equation to be used here is:

x = v₀t + 1/2 at²
where
x is the distance
v₀ is the initial velocity
a is the acceleration

In order to solve this, let's assume the object is free falling. So v₀ = 0 and a = 9.81 m/s².

x = 0 + 1/2 (9.81)(3)²
x = 44.145 meters

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2 years ago

In a first-order decomposition reaction, 50.0% of a compound decomposes in 10.5 min.

mihalych1998 [28]

In this reaction 50% of the compound decompose in 10.5 min thus, it is half life of the reaction and denoted by symbol $t_{1/2}$ .

(a) For first order reaction, rate constant and half life time are related to each other as follows:

$k=\frac{0.6932}{t_{1/2}}=\frac{0.6932}{10.5 min}=0.066 min^{-1}$

Thus, rate constant of the reaction is $0.066 min^{-1}$ .

(b) Rate equation for first order reaction is as follows:

$k=\frac{2.303}{t_{1/2}}log\frac{[A_{0}]}{[A_{t}]}$

now, 75% of the compound is decomposed, if initial concentration $[A_{0} ]$ is 100 then concentration at time t $[A_{t} ]$ will be 100-75=25.

Putting the values,

$0.066 min^{-1}=\frac{2.303}{t}log\frac{100}{25}=\frac{2.303}{t}(0.6020)$

On rearranging,

$t=\frac{2.303\times 0.6020}{0.066 min^{-1}}=21 min$

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8 0

3 years ago

The ion MnOis often used to analyze for the Fe2+ content of an aqueous solution by using the (unbalanced) reaction Mno+Fe2+ + Fe

dusya [7]

Answer:

B) 0.230 M

Explanation:

The first step is to <u>balance the reaction</u> between the Ferrous ion and the permanganate ion:

$5~Fe^+^2~+~MnO_4^-^1~+~8H^+~->~5Fe^+^3~+~Mn^+^2~+4H_2O$

Then we have to <u>calculate the moles</u> of $MnO_4^-$ :

$M~=~\frac{mol}{L}$

$mol~=~M*L$

$mol~=~0.033~M*0.0633L=~0.002088~mol~MnO_4^-$

Then using the <u>molar ratio</u> we can find the moles of $Fe^+^2$ :

$0.002088~mol~MnO_4^-\frac{5~mol~Fe^+^2}{1~mol~MnO_4^-}=0.01044~mol~Fe^+^2$

Finally we can calculate the molarity:

$M=\frac{0.01044~mol~Fe^+^2}{0.0455~L}=0.230~M$

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3 years ago

How will the concentration of H+ and OH− ions change when a substance with a pH 3.2 is added to water? Both H+ and OH− will incr

Lunna [17]

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2 years ago

Read 2 more answers