1) What is the mass of a CO2 gas sample that occupies 5.60 L at STP? 2) Which of

Question

1) What is the mass of a CO2 gas sample that occupies 5.60 L at STP?

2) Which of the following statements are correct? (Select all that apply).

a Two moles of chlorine gas at 20 °C is heated to 250 °C while the volume is kept constant. The density of the gas increases.
b According to Boyle's Law; if the pressure applied to an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is halved.
c Under the same pressure and temperature; the volume of 2 mol of O2 gas is larger than that of 2 mol of N2 gas.
d According to Charles's Law; if the temperature (in K) of an ideal gas sample is doubled while other conditions stay the same; the volume of the sample is doubled.
e According to Avogadro's Law; if 0.35 mol of an ideal gas sample has a volume of 7.84 L; the volume of 1.05 mole of the gas is 23.5 L at the same temperature and pressure.

1) What is the mass of a CO2 gas sample that occupies 5.60 L at STP?

Explanation / Answer

1. any gas ta STP occupies 22.4 L per mol

so

mol of 5.6 L --- 5.6/22.4 = 0.25 mol of CO2

mass = mol*MW = 0.25*44 = 11 g of CO2

Q2

a) 2 moles of Cl2 gas at 20C to 250 C = this is false, since volume is fixed, so d = m/V will remain the same

b) boyle law state PV ratio, so if we doulbe P, then V must be halved is true

c) True, since all mol of gases are similar (in ideal gas law) at same conditions

d) Charles law states V/T ratios, if we increase T, then expect V to doulbe, this is true

e)

1 mol = 22.4 L so 0.35 mol = 22.4*0.35 = 7.84 true

for 1.05 mol = 1.05*22.4 = 23.52 true as well

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