The molecular mass of is:
2·1 + 1·32 + 4·16 = 98 g/mol
The amount of solute, expressed by mol, is:
The molar concentration definition is:
Doing the calculations:
(If you detect any mistakes in my English report me them, please).
Which of the following correctly
1 answer:
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The pressure exerted by 0.57 moles of CO2 at a temperature of 25°C and a volume of 500 ml is 28 atm.
<u>Explanation:</u>
According to ideal gas law,
PV = nRT
where P represents the pressure of a gas,
V represents the volume of a gas,
n represents the number of moles,
R represents the gas constant = 0.0821 L atm / mol K.
T represents the temperature of a gas.
Given V = 500 ml = 0.5 l, T = 25°C = 298 K, n = 0.57 mol
PV = nRT
P = nRT / V
= (0.57 0.0821
298) / 0.5
P = 28 atm.
The pressure of a gas is 28 atm.