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geniusboy [140]
3 years ago
5

If the temperature of a gas is raised from 30°C to 60°C, what happens to the pressure?

Chemistry
1 answer:
Fofino [41]3 years ago
5 0
<h3>Answer:</h3>

The pressure increases by 10% of the original pressure

Thus the new pressure is 1.1 times the original pressure.

<h3>Explanation:</h3>

We are given;

  • Initial temperature as 30°C, but K = °C + 273.15
  • Thus, Initial temperature, T1 =303.15 K
  • Final temperature, T2 is 333.15 K

We are required to state what happens to the pressure;

  • We are going to base our arguments to Pressure law;
  • According to pressure law, the pressure of a gas and its temperature are directly proportional at a constant volume
  • That is; P α T
  • Therefore, at varying pressure and temperature

\frac{P1}{T1}=\frac{P2}{T2}

Assuming the initial pressure, P1 is P

Rearranging the formula;

[tex]P2=\frac{P1T2}{T1}[/tex]

P2=\frac{(P)(333.15K)}{303.15K}

     P2 = 1.099P

                 = 1.10 P

The new pressure becomes 1.10P

This means the pressure has increased by 10%

We can conclude that, the new pressure will be 1.1 times the original pressure.

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Calculate the number of moles equivalent to 12.7 gram of iodine molecule ​
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\LARGE{ \boxed{ \purple{ \rm{Answer}}}}

☃️ Chemical formulae ➝ \sf{I_2}

How to find?

For solving this question, We need to know how to find moles of solution or any substance if a certain weight is given.

\boxed{ \sf{No. \: of \: moles =  \frac{Given \: weight}{Molecular \: weight} }}

Solution:

❍ Molecular weight of \sf{I_2}

= 2 × 126.90

= 253.80

= 254 (approx.)

❍ Given weight: 12.7

Then, no. of moles,

⇛ No. of moles = 12.7 / 254

⇛ No. of moles = 0.05 moles

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<u>━━━━━━━━━━━━━━━━━━━━</u>

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Volume is calculated as follow;

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x = 3680

x = 3680 * 3.48 / 100

x = 128.064 L

Number of moles = Mass / Molar mass

Mass = Density *  Volume

Mass = 804 * 128.064 = 102963.456 g

Number of moles = 102963.456 / 184.37

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