# A quantity of #N_2# gas originally held at 4.75 am in a 1.00L container at 26°C is transferred to a 10.0 L container at 20°C. What is the total pressure in the new container?

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Also, a quantity of #O_2# gas originally at 5.25 atm and 26°C in a 5.00 L container is transferred to this same container.

Also, a quantity of

##### 1 Answer

#### Explanation:

Notice that the *volume* and the *temperature* of the gas change when going from the first container to the second container, but that the *number of moles* of gas remains **constant**.

This tells you that you can use the combined gas law equation to find the change in *pressure*

#color(blue)((P_1V_1)/T_1 = (P_2V_2)/T_2)" "# , where

Notice that the **volume** of the container *increases* by a factor of **decreases**. Both these changes allow you to precit that the pressure of the gas will be **smaller** in the second container.

Plug your values and solve for **do not** forget to convert the temperature from *degrees Celsius* to *Kelvin*!

#P_2 = V_1/V_2 * T_2/T_1 * P_1#

#P_2 = (1.00 color(red)(cancel(color(black)("L"))))/(10.0color(red)(cancel(color(black)("L")))) * ( (273.15 + 20)color(red)(cancel(color(black)("K"))))/( (273.15 + 26)color(red)(cancel(color(black)("K")))) * "4.75 atm"#

#P_2 = "0.4655 atm"#

You *should* round this off to one sig fig, the number of sig figs you have for the temperature of the gas in the second container, but I'll leave it rounded to two sig figs

#P_2 = color(green)("0.47 atm")#

I'll leave the second part of the problem, the one with the sample of oxygen, to you as practice.