6. A 0.110 mol sample of an ideal gas Occupies 3.50L. What is the volume of 0.25

Question

6. A 0.110 mol sample of an ideal gas Occupies 3.50L. What is the volume of 0.250 moles of this gas at the same temperature and pressure? 7. What is the volume of 0.2500 moles of an ideal gas at 1.20 atm and 350.0K? How many neon atoms will occupy 3.20 L at 20.0 degree C and 715.0 mm. Hg.? 10. What are the major assumptions that separate an ideal gas from a real gas? 11. What volume of carbon dioxide will be formed at 25.0 degree C and 1.10atm from the reaction of 3.00g of sodium carbonate with excess hydrochloric acid?

Explanation / Answer

6. Avagadro's Law

V1/n1 = V2/n2

3.50 L/0.110 mol = V2/0.250 mol

V2= 7.95 L

7. Ideal gas law

PV=nRT

V = nRT/P = (0.2500mol)(0.0821 Latm/molK)(350.0 K)/(1.20 atm) = 5.99 L

8. Ideal gas law

PV=nRT

n=PV/(RT) = (715.0 mmHg/ (760 mmHg/1atm))(3.20 L)/((0.0821 Latm/molK)(20+273 K) = 0.125 mol

0.125 mol x (6.022 x 1023 atoms/mol) = 7.54 x 1022 atoms

10. In an ideal gas, particles move randomly and collide without any kind of interaction. This is not true in reality since gas molecules have intermolecular forces. Heavier molecules tend to deviate from an ideal gas more than smaller molecules. Gases behave more like an ideal gas at higher temperature and lower pressure, since the intermolecular attractions become less significant compared to the particle's kinetic energy.

11. Na2CO3 + 2HCl --> 2NaCl + H2O + CO2

n = (3.00 g Na2CO3) / (105.99 g/mol) / (1 mol CO2/1 mol Na2CO3) = 0.0283 mol Na2CO3

PV=nRT

V=nRT/P = (0.0283 mol)(0.0821 Latm/molK)(25+273 K)/(1.10 atm) = 0.629 L

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