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Firdavs [7]
2 years ago
6

In order to get lots of helium into tanks to fill kiddy balloons, they put force or pressure onto it. If i have 595 liters of he

lium at 1.00 atmosphere of pressure (that’s normal air pressure, or the pressure of the air), then what volume would it have if i applied 55.0 atmospheres of force or pressure to it?
Chemistry
1 answer:
alexandr402 [8]2 years ago
5 0

Answer:

1.90 L

Explanation:

Using Boyle's law  

{P_1}\times {V_1}={P_2}\times {V_2}

Given ,  

V₁ = 595 L  

V₂ = ?

P₁ = 1.00 atm

P₂ = 55.0 atm

Using above equation as:

{P_1}\times {V_1}={P_2}\times {V_2}

{1.00}\times {595}={55.0}\times {V_2}

{V_2}=\frac{{1.00}\times {595}}{55.0}\ L

{V_2}=1.90\ L

<u>The volume would be 1.90 L.</u>

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  • V_1=49.8mL
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Using Charles law

\\ \sf\longmapsto V_1T_2=V_2T_1

\\ \sf\longmapsto V_2=V_1T_2\div T_1

\\ \sf\longmapsto V_2=\dfrac{49.8(356)}{291}

\\ \sf\longmapsto V_2=\dfrac{17728.8}{291}

\\ \sf\longmapsto V_2=60.9mL

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A reaction has activation energy of 85kjper mol. What is the effect on the rate of raising the temperature from 20degree to 30 d
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Explanation:

According to Arrhenius equation with change in temperature, the formula is as follows.

ln \frac{k_{2}}{k_{1}} = \frac{-E_{a}}{R}[\frac{1}{T_{2}} - \frac{1}{T_{1}}]

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ln \frac{k_{2}}{k_{1}} = \frac{-85\times 1000J/mol}{8.314J/Kmol}[\frac{1}{303} - \frac{1}{293}]

ln \frac{k_{2}}{k_{1}}=1.15

\frac{k_{2}}{k_{1}}=3

Thus rate increases 3 times on raising the temperature from 20degree to 30 degree​

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