Question

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law? Which sample contains more molecules: 2.0 L of Cl2 at STP or 3.0 L of CH at 300K and 1150 mmHg? Which sample weighs more? Which sample contains more molecules: 2.0L of CO2 at 300 K and 500 mmHg or 1.5 L of N2 at 57 °C and 760 mmHg? Which sample weighs more? 8.78 8.79 8.80 If 2.3 mol of He has a volume of 0.15 L at 294 K, what is in atm? In psi? the pressure If 3.5 mol of O2 has a volume of 27.0 L at a pressure of 1.6 atm, what is its temperature in degrees Celsius? 8.81 If 15.0 g of CO2 gas has a volume of 0.30 L at 310 K, what is its pressure in mmHg? If 20.0 g of N gas has a volume of 4.00 L and a pressure of 6.0 atm, what is its temperature in degree Celsius? 8.82 8.83

Answer 1

Using ideal gas equation,

At STP, moles of Cl2 = 2.0/22.4=> 0.0893 mol

Moles of CH4 = PV/RT

=1150×3/0.0821×300×760

=> 0.184 mol

Number of Cl2 molecules = 0.0893× 6.022×10²³

=> 5.38×10²² molecules

Mass of Cl2 = 0.0893×71 => 6.34 g

Number of CH4 molecules = 0.184×6.022×10²³ =>1.11×10²³ molecules

Mass of CH4 = 16×0.184=> 2.94 g

So CH4 contains more molecules

And Cl2 has more mass

2) moles of CO2 = 2×500/760×0.0821×300

= 0.0534 moles

Number of CO2 molecules = 0.0534×6.022×10²³=>3.2×10²² molecules

Mass if CO2 = 0.0534×44 => 2.35 g

Moles of N2 = 1.5×1/0.0821×330=0.055 mol

Molecules of N2 = 0.055×6.022×10²³ = 3.33×10²² molecules

Mass of N2 = 0.055×28 => 1.38 g

N2 has more molecules and CO2 has more mass.

3) using ideal gas equation,

P = nRT/V

=2.3×0.0821×294/0.15

= 370.1 atm = 5439 psi

4) T = 27×1.6/0.0821×3.5

=> -122.7 °c

5) P = 15×0.0821×310/0.3×44

= 28.9 atm

= 21964 mm of Hg

5) T = 4.0×6×28/0.0821×20

= 136.3 °c