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3 years ago

Determine the volume in liters occupied by 22.6 g of I2 gas at STP.

Chemistry

1 answer:

AleksandrR [38]3 years ago

6 0

The volume in liters occupied by 22.6 g of I₂ gas at STP is 1.99 L (answer A)

calculation

Step: find the moles of I₂

moles= mass÷ molar mass

from periodic table the molar mass of I₂ is 253.8 g/mol

moles = 22.6 g÷253.8 g/mol =0.089 moles

Step 2:find the volume of I₂ at STP

At STP 1 moles =22.4 L

0.089 moles= ? L

by cross multiplication

={ (0.089 moles x 22.4 L) /1 mole} = 1.99 L

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The activation energy of an uncatalyzed reaction is 70 kJ/mol. When a catalyst is added, the activation energy (at 20 °C) is 42

denis23 [38]

Answer:

T = 215.33 °C

Explanation:

The activation energy is given by the Arrhenius equation:

$k = Ae^{\frac{-Ea}{RT}}$

Where:

k: is the rate constant

A: is the frequency factor

Ea: is the activation energy

R: is the gas constant = 8.314 J/(K*mol)

T: is the temperature

We have for the uncatalyzed reaction:

Ea₁ = 70 kJ/mol

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Ea₂ = 42 kJ/mol

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The frequency factor A is constant and the initial concentrations are the same.

Since the rate of the uncatalyzed reaction (k₁) is equal to the rate of the catalyzed reaction (k₂), we have:

$k_{1} = k_{2}$

$Ae^{\frac{-Ea_{1}}{RT_{1}}} = Ae^{\frac{-Ea_{2}}{RT_{2}}}$ (1)

By solving equation (1) for T₁ we have:

$T_{1} = \frac{T_{2}*Ea_{1}}{Ea_{2}} = \frac{293 K*70 kJ/mol}{42 kJ/mol} = 488. 33 K = 215.33 ^\circ C$

Therefore, we need to heat the solution at 215.33 °C so that the rate of the uncatalyzed reaction is equal to the rate of the catalyzed reaction.

I hope it helps you!

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