1. W hich of the following gases experiences the greatest degree of deviation fr
ID: 580348 • Letter: 1
Question
1. W hich of the following gases experiences the greatest degree of deviation from (A) CH (B) 0 (C) N2 temperatures? east amoun SeO2 Of Pactcle s uppose you had 1.0 mol samples the following gases at STP. If the volume of . each of the samples of gas was reduced to one tenth of its original size and the remained the same, which gas would have the lowest pressure? He (B) Kr east amount (D) NO (E) 02 3. An excess of Na (s) is added to 100 mL of 0.8 MHCI at STP. What volume of H gas can be produced? (A) 8.96L 0.896 L 7.9 L 1.79 L 22.4 L Real gases behave like ideal gases at higher temperatures and lower pressures because: 4. (A) Collisions between gas particles are less frequent TB)Collisions between gas particles become less elastic. (C) Intermolecular attractions decrease. (D) The average distance between gas particles increases. (B) Collisions between gas particles and the sides of the container become less elastic.Explanation / Answer
3. At high pressure and low temperatures the intermolecular forces between the gas particles, causes significant deviation from ideal behaviour.
SeO2 will show greatest degree of deviation.
2. PV = nRT
Temperature same
n = 1 mole = mass/molar mass
n = m/M
V = V/10
P = 10mRT/MV
This means the pressure is inversely proportional to Molar mass of the gas
The gas with highest molar mass will have the lowest pressure
Hence Kr = 83.79g/mol
Kr will have lowest pressure
Answer is B
3. Moles of HCl used = 0.8 M x 0.100L = 0.08 moles
2Na(s) + 2HCl(aq) ----à 2NaCl (aq) + H2(g)
According to the equation:
2 moles of HCl produces H2 = 1 mole
So, 0.08 moles of HCl will produce H2 = 0.08/2 = 0.04 moles
At STP
T = 273 K
P = 1 atm
R = 0.08206 L. atm/mol.K
PV = nRT
V = nRT/P
V = (0.04 moles x 0.08206 L. atm/mol.K x 273.15 K)/(1 atm)
V = 0.896 L
Answer is A.
4.Answer is D
At high temperature the gas particles have high kinetic energy and they collide with each and walls of the container (elastic collision). The intermolecular forces between the gas particles is low, they are far apart and average distance between the particles increases.
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