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user100 [1]
4 years ago
6

A sample of a gas in a rigid container has an initial pressure of 1.049 kPa and an initial temperature of 7.39 K. The temperatur

e is increased to 30.70 K. What is the new pressure?
Chemistry
1 answer:
Doss [256]4 years ago
5 0

Answer:- 4.36 kPa

Solution:- At constant volume, the pressure of the gas is directly proportional to the kelvin temperature.

\frac{P_1}{T_1}=\frac{P_2}{T_2}

Where the subscripts 1 and 2 are representing initial and final quantities.

From given data:

P_1 = 1.049 kPa

P_2 = ?

T_1 = 7.39 K

T_2 = 30.70 K

For final pressure, the equation could also be rearranged as:

P_2=\frac{P_1T_2}{T_1}

Let's plug in the values in it:

P_2=\frac{1.049kPa(30.70K)}{7.39K}

P_2 = 4.36 kPa

So, the new pressure of the gas is 4.36 kPa.

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The equation for the reaction between KOH and HCl is as follows
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the number of HCl moles reacted = number of KOH moles reacted 
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0.2 mol of HCl in - 1000 cm³
Therefore volume required for 0.015 mol = 1000 cm³ / 0.2 mol * 0.015 mol 
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