s of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g.°C) C) 6.90 L sample of nitrogen N₂ is 7 L at 38°C and 740 torr. What volume will it occupy at STP? B) 7.18 L D)5.98 L L sity of NH3 at 4 atm pressure and a temperature of 30°C? C) 3.36 g/L B) 1.39 g/L t is required to raise the temperature of 1.5 g of water from 25°C to 29°C? kJ B) 6.27 kJ D) 40.5 kJ C) 25.1 kJ D) 634 K temperature where AG=0 for the following reaction: (Given: AH = -155 kJ and /K) CAUTION: Beware of units.NH,(g) + HCl(g)---> NH₂Cl(s) R) 545 K C) 467 K D) 2.73 g/L
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![An
(molar mass of H-1, N-14g/mol), (R-0.0821 L.atm/K.mol), (The specific heat of water is 4.184J/g.°C)]
1) The volume of a sample of nitrogen N2 is 7 L at 38°C and 740 torr. What volume will it occupy at STP?
A) 7.78 L
B) 7.18 L
D)5.98 L
C) 6.90 L
2) What is the density of NH3 at 4 atm pressure and a temperature of 30°C?
A) 16.6 g/L
C) 3.36 g/L
B) 1.39 g/L
D) 2.73 g/L
3) How much heat is required to raise the temperature of 1.5 g of water from 25°C to 29°C?
A) 12.55 kJ
B) 6.27 kJ
C) 25.1 kJ
D) 40.5 kJ
4) Estimate the temperature where AG - 0 for the following reaction: (Given: AH = -155 kJ and
AS = -284.5 J/K) CAUTION: Beware of units.NH3(g) + HCl(g)-NH.CI(s)
A) 685 K
B) 545 K
C) 467 K
D) 634 K
5) Calculate AH° for the reaction:
(1) CO+Hz
(2)CO ) +H_O»
(3) CO(g) + 3H2(g) →
A) 33 kJ
6) Calculate AG for the reaction
CO(g)
CO2(g)
CO) + 1/2O2() -
A) 217.2 kJ
Which is the strongest
A) Dipole-dipole
2C+2H2O --->
C) + H₂O
H2(g) + CO2(g)
CH48) + H₂O(g)
B) 53 kJ
C(s) + 1/2O2(g)
C()+ O2(g)
CO2(g)
CH4(g) + CO2(g)
AH-140 kJ
AH 41kJ
ΔΗ°=-206kJ
C) -372 kJ
AG° = ??
AG = 454.4 kJ
AG = -237.2 kJ
C) 197.2 kJ
B)-265.8 kJ
D) 651.6 kJ
D) London
C) Ionic bonding
intermolecular force among a group of molecules of comparable molar mass?
B) Hydrogen bonding
7)
8) Which of the following pure substances exhibits hydrogen
A) HCI
B) H₂S
D) -116 kJ
C) NH3
bonding?
D) CH4
9) A solution was made by dissolving 3.15 g of a solute in
120.3 g of acetone. The solution boiled at
56.58° C. The boiling point of pure acetone is 55.95° C, and the Kb -1.71° C/m. What is the molecular
weight of the solute?
A) 140
B) 105
C) 12.7
D) 71.1
D) 9.34 kg
10) What mass of ethylene glycol (M.W. = 62.1 g/mol) antifreeze must be added to 12.0 liters of water to
C) 0.78 kg
produce a solution that freezes at -23.3 C degrees. Density of water is 1 g/ml and Kr= 1.86° C/m.
B) 3.41 g
A) 6.22 Kg](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbfaea92a-9638-4015-ac2a-6c50f8cc86a5%2Fa79b5b66-6a69-4dd1-ab1a-d80654848907%2Ff651g9fn_processed.jpeg&w=3840&q=75)
STP means standard temperature pressure. Standard temperature is 273 Kelvin and standard pressure is one atmosphere or 760 torr. We have to calculate volume at STP..
Step by step
Solved in 4 steps with 1 images
