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kirza4 [7]
3 years ago
11

Consider the reaction, X + 2Y → XY2 If X and Y are completely consumed in the reaction and we start with 10.0 mol of Y, then how

many total moles of X and Y will be in the reaction?
Physics
1 answer:
Harrizon [31]3 years ago
3 0

Answer:

In the reaction you would have 15.0 mols of Y and X.

Explanation:

The stoichiometric coefficents for X and Y are 1 and 2 respectively, if you start the reaction with 10.0 moles of Y you would need 5.0 moles of X in order to achieve a complete reaction so you will have 15.0 total moles in the reaction, assuming no mass loss and no nuclear reactions.

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ololo11 [35]

Answer:

a)

a = 1/5

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b)

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y(1/3) = 2.598

c)

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d)

x'(1/3) = -13.603

Explanation:

Hi!

a)

We can notice that

x(t)/5 = cos(πt)

y(t)/3 = sin(πt)

Therefore:

( x(t) / 5 )^2 + ( y(t) / 3 )^2 = cos^2(πt) + sin^2(πt) = 1

That is:

a = 1/5

b = 1/3

b)

At t=1/3

x(1/3) = 5 cos(π/3)

y(1/3) = 3 sin(π/3)

But

cos(π/3) = 1/2 = 0.5

sin(π/3) = √3 / 2 = 0.866

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x(1/3) = 2.5

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c)

The horizontal velocity is:

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d)

at time t =1/3

x'(1/3) = -5π sin(π/3) = -13.603

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jeka94

Answer:

426.84 m

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