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3 years ago

The atmospheric pressure in Denver, Colorado, is usually about 84.00 kPa. What is this pressure in atm and torr units?

Chemistry

1 answer:

tresset_1 [31]3 years ago

7 0

Answer:

84.00 kPa = 630.084 torr

Formula for kPa to torr: For an approximate result, multiply the pressure value by 7.501. 84* 7.501

84.00 kPa = 0.831683168 atm

Formula for kPa to atm: for an approximate result, divide the pressure value by 101. 84/101

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A sample of hellium has a volume of 500 mL at STP. What will be its new volume be in mL if the temperature is increased to 325 K

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$V_2=482.5mL$

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to solve this problem by using the combined gas law due to the fact that we are dealing with variable volume, temperature and pressure:

$\frac{P_2V_2}{T_2}=\frac{P_1V_1}{T_1}$

In such a way, we solve for the final volume, V2, considering that the initial volume, V1, is 500 mL, the initial temperature, T1, is 273 K (STP), the initial pressure, P1, is 1 atm (STP) and the final temperature, T2, is 325 K and the final pressure, P2, is 125 kPa (1.23 atm):

$V_2=\frac{P_1V_1T_2}{T_1P_2} \\\\V_2=\frac{(1atm)(500mL)(325K)}{(273K)(1.23atm)} \\\\V_2=482.5mL$

Regards!

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3 years ago