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lions [1.4K]
3 years ago
7

The partial pressure of cartbon dioxide in the atmgsphere is 0239 toer Caiculate the partial pressure in mm He and atm Rpund eac

h of your answers to 3 significant cigits ate
Chemistry
1 answer:
Verizon [17]3 years ago
3 0

Answer :

The pressure of carbon dioxide in the atmosphere in mmHg is 0.239mmHg.

The pressure of carbon dioxide in the atmosphere in atm is 3.14\times 10^{-4}atm.

Explanation :

The conversion used for pressure from torr to mmHg is:

1 torr = 1 mmHg

The conversion used pressure from torr to atm is:

1 atm = 760 torr

or,

1torr=\frac{1}{760}atm

As we are given the pressure of carbon dioxide in the atmosphere 0.239 torr. Now we have to determine the pressure of carbon dioxide in the atmosphere in mmHg and atm.

<u>Pressure in mmHg :</u>

As, 1torr=1mmHg

So, 0.239torr=\frac{0.239torr}{1torr}\times 1mmHg=0.239mmHg

Thus, the pressure of carbon dioxide in the atmosphere in mmHg is 0.239mmHg.

<u>Pressure in atm:</u>

As, 1torr=\frac{1}{760}atm

So, 0.239torr=\frac{0.239torr}{1torr}\times \frac{1}{760}atm=3.14\times 10^{-4}atm

Thus, the pressure of carbon dioxide in the atmosphere in atm is 3.14\times 10^{-4}atm.

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