Q. How many significant figures are in the number 0.007890?
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Solution
The significant figures are 7, 8, 9, and the trailing zero counts.
Correct Answer: C — 5
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Q. How many significant figures are in the number 100.0?
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Solution
The trailing zero after the decimal point counts as a significant figure.
Correct Answer: D — 4
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Q. How many significant figures are in the number 1002?
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Solution
All non-zero digits are significant, so 1002 has 4 significant figures.
Correct Answer: C — 4
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Q. How many significant figures are in the number 5000 when no decimal point is present?
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Solution
5000 has 1 significant figure unless specified otherwise (e.g., 5000. has 4 significant figures).
Correct Answer: A — 1
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Q. How many significant figures are in the number 5000?
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Solution
5000 has 1 significant figure unless specified with a decimal point (e.g., 5000. has 4).
Correct Answer: A — 1
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Q. How much heat is required to convert 1 kg of water at 100°C to steam at 100°C? (Latent heat of vaporization = 2260 J/g)
A.
1000 J
B.
2260 J
C.
2260000 J
D.
100000 J
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Solution
Q = m * L = 1000 g * 2260 J/g = 2260000 J.
Correct Answer: C — 2260000 J
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Q. How should the number 0.0001234 be rounded to two significant figures?
A.
0.00012
B.
0.00013
C.
0.0001
D.
0.000123
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Solution
To round 0.0001234 to two significant figures, we look at the first two non-zero digits (1 and 2) and round up, resulting in 0.00013.
Correct Answer: B — 0.00013
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Q. How should the number 0.05060 be rounded to three significant figures?
A.
0.051
B.
0.0506
C.
0.05060
D.
0.050
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Solution
To round 0.05060 to three significant figures, we keep the first three significant digits (5, 0, and 6), resulting in 0.0506.
Correct Answer: B — 0.0506
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Q. If 1 kg of water is heated from 20°C to 100°C, how much heat is absorbed? (Specific heat of water = 4.2 J/g°C)
A.
3360 J
B.
4000 J
C.
4200 J
D.
4800 J
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Solution
Q = m*c*ΔT = 1000 g * 4.2 J/g°C * (100°C - 20°C) = 4200 J.
Correct Answer: C — 4200 J
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Q. If 1 mole of an ideal gas occupies 22.4 L at STP, what is the pressure exerted by the gas?
A.
1 atm
B.
2 atm
C.
0.5 atm
D.
4 atm
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Solution
At STP (Standard Temperature and Pressure), 1 mole of an ideal gas occupies 22.4 L at a pressure of 1 atm.
Correct Answer: A — 1 atm
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Q. If 1 mole of an ideal gas occupies 22.4 L at STP, what is the volume occupied by 2 moles at the same conditions?
A.
11.2 L
B.
22.4 L
C.
44.8 L
D.
56.8 L
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Solution
According to Avogadro's Law, 2 moles of gas will occupy double the volume, which is 44.8 L at STP.
Correct Answer: C — 44.8 L
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Q. If 100 g of water at 0°C is mixed with 100 g of water at 100°C, what will be the final temperature?
A.
50°C
B.
25°C
C.
75°C
D.
0°C
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Solution
The final temperature will be 50°C due to equal masses and specific heat capacities.
Correct Answer: A — 50°C
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Q. If 100 g of water at 0°C is mixed with 100 g of water at 100°C, what will be the final temperature of the mixture?
A.
50°C
B.
25°C
C.
75°C
D.
0°C
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Solution
Using the principle of conservation of energy, the final temperature will be 50°C.
Correct Answer: A — 50°C
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Q. If 100 g of water at 80°C is mixed with 200 g of water at 20°C, what will be the final temperature?
A.
30°C
B.
40°C
C.
50°C
D.
60°C
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Solution
Using the principle of conservation of energy, the final temperature can be calculated to be 40°C.
Correct Answer: B — 40°C
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Q. If 100 J of heat is added to a system and 40 J of work is done by the system, what is the change in internal energy?
A.
60 J
B.
40 J
C.
100 J
D.
140 J
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Solution
According to the First Law of Thermodynamics, ΔU = Q - W. Here, ΔU = 100 J - 40 J = 60 J.
Correct Answer: A — 60 J
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Q. If 10^(2x) = 100, what is the value of x?
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Solution
100 = 10^2, so 2x = 2, hence x = 1.
Correct Answer: B — 0.5
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Q. If 10^x = 0.01, what is the value of x?
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Solution
Since 0.01 = 10^(-2), we have x = -2.
Correct Answer: A — -2
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Q. If 2 moles of an ideal gas at 300 K occupy a volume of 10 L, what is the pressure of the gas? (Use R = 0.0821 L·atm/(K·mol))
A.
0.5 atm
B.
1.0 atm
C.
2.0 atm
D.
3.0 atm
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Solution
Using the Ideal Gas Law, P = nRT/V = (2 moles * 0.0821 L·atm/(K·mol) * 300 K) / 10 L = 4.926 atm.
Correct Answer: B — 1.0 atm
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Q. If 200 g of ice at 0°C is added to 100 g of water at 80°C, what will be the final temperature of the mixture? (Latent heat of fusion of ice = 334 J/g)
A.
0°C
B.
20°C
C.
40°C
D.
60°C
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Solution
Heat lost by water = Heat gained by ice. 100g * 80°C = 200g * 334 J/g + 200g * (Tf - 0°C). Solving gives Tf = 20°C.
Correct Answer: B — 20°C
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Q. If 2^(x+1) = 16, what is the value of x?
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Solution
16 = 2^4 => x + 1 = 4 => x = 3
Correct Answer: B — 3
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Q. If 300 g of water at 25°C is mixed with 200 g of water at 75°C, what is the final temperature? (Specific heat of water = 4.2 J/g°C)
A.
40°C
B.
50°C
C.
60°C
D.
70°C
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Solution
Using m1*T1 + m2*T2 = (m1 + m2)*Tf, we find Tf = (300*25 + 200*75) / (300 + 200) = 50°C.
Correct Answer: B — 50°C
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Q. If 3^(2x) = 81, what is the value of x?
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Solution
Since 81 = 3^4, we have 3^(2x) = 3^4, thus 2x = 4, giving x = 2.
Correct Answer: A — 2
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Q. If 4^x = 64, what is the value of x?
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Solution
Since 64 = 4^3, we have x = 3.
Correct Answer: B — 3
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Q. If 500 J of heat is added to a system and 200 J of work is done by the system, what is the change in internal energy?
A.
300 J
B.
500 J
C.
700 J
D.
200 J
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Solution
According to the first law of thermodynamics, ΔU = Q - W. Here, ΔU = 500 J - 200 J = 300 J.
Correct Answer: A — 300 J
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Q. If 5^(x+1) = 125, what is the value of x?
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Solution
125 = 5^3, so x + 1 = 3, hence x = 2.
Correct Answer: B — 2
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Q. If 5^(x-1) = 25, what is the value of x?
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Solution
Since 25 = 5^2, we have 5^(x-1) = 5^2, thus x - 1 = 2, giving x = 3.
Correct Answer: A — 2
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Q. If 5^x = 125, what is the value of x?
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Solution
125 = 5^3 => x = 3
Correct Answer: C — 3
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Q. If 5^x = 25, what is the value of x?
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Solution
Since 25 = 5^2, we have 5^x = 5^2, thus x = 2.
Correct Answer: B — 2
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Q. If 7^(x) = 49, what is the value of x?
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Solution
49 = 7^2, so x = 2.
Correct Answer: B — 2
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Q. If 8^(x) = 64, what is the value of x?
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Solution
64 = 8^2, so x = 2.
Correct Answer: B — 2
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