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 
.
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,
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, 
So, 
Thus, the pressure of carbon dioxide in the atmosphere in mmHg is 0.239mmHg.
<u>Pressure in atm:</u>
As,
So, 
Thus, the pressure of carbon dioxide in the atmosphere in atm is .
Mass number minus atomic number equals neutrons.
234-92=142
The volume of Sulfur dioxide-SO₂ at STP : = 102.144 L
<h3>Further explanation</h3>
Given
4.56 mol Sulfur dioxide-SO₂
Required
The volume
Solution
Conditions at T 0 ° C and P 1 atm are stated by STP (Standard Temperature and Pressure). At STP, Vm is 22.4 liters/mol.
so for 4.56 mol :
= 4.56 x 22.4 L
= 102.144 L
Bacteria are the living/biotic components in an ecosystem.
<span>Avogadro's number
represents the number of units in one mole of any substance. This has the value
of 6.022 x 10^23 units / mole. This number can be used to convert the number of
atoms or molecules into number of moles. We calculate as follows:
0.340 mol Br2 ( </span>6.022 x 10^23 molecules / mol ) = 2.05 x 10^23 molecules
