Chapter 8: Q. 8.73 (page 282)

A sample of Hydrogen $(H_{2})$ gas at $127 ° C$ has a pressure of $2.00 a t m$ . at final temperature, in degrees Celcius, will the pressure of the $H_{2}$ decreases to $0.25 a t m$ , if $V a n d n$ do not change?

Short Answer

Expert verified

The final temperature of $H_{2}$ will be $- 223 ° C$ .

Step by step solution

Given Information

We have given the temperature is $127 ° C$ and pressure is $2.00 a t m$ of Hydrogen $(H_{2})$ .

Simplify

According to the question, there will be no change in the amount of gas and the volume of the gas will also be constant.

Using combined gas law

$\frac{p_{1} V_{1}}{T_{1}} = \frac{p_{2} V_{2}}{T_{2}}$

We can see, the pressure is directly related to the temperature.

So,

role="math" localid="1652528887995" $T_{2} = \frac{P_{2} T_{2}}{P_{1}} = \frac{0.25 a t m \times 400 K}{2 a t m} T_{2} = 50 K T_{2} = (50 - 273) ° C = - 223 ° C$

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A sample of Hydrogen $(H_{2})$ gas at $127 ° C$ has a pressure of $2.00 a t m$ . at final temperature, in degrees Celcius, will the pressure of the $H_{2}$ decreases to $0.25 a t m$ , if $V a n d n$ do not change?

Short Answer

Step by step solution

Given Information

Simplify

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A sample of HydrogenH2gas at 127°Chas a pressure of 2.00atm. at final temperature, in degrees Celcius, will the pressure of the H2decreases to 0.25atm, if Vandndo not change?

Short Answer

Step by step solution

Given Information

Simplify

One App. One Place for Learning.

Most popular questions from this chapter

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Study anywhere. Anytime. Across all devices.

A sample of Hydrogen $(H_{2})$ gas at $127 ° C$ has a pressure of $2.00 a t m$ . at final temperature, in degrees Celcius, will the pressure of the $H_{2}$ decreases to $0.25 a t m$ , if $V a n d n$ do not change?