Q. What is the molar mass of the product formed when 1 mole of Mg reacts with 2 moles of HCl?
A.
24.3 g
B.
36.5 g
C.
58.5 g
D.
74.5 g
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Solution
Mg + 2HCl → MgCl2 + H2. Molar mass of MgCl2 = 24.3 + 2*35.5 = 95.3 g.
Correct Answer: D — 74.5 g
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Q. What is the molar mass of the product formed when 1 mole of nitrogen reacts with 3 moles of hydrogen?
A.
28 g
B.
14 g
C.
32 g
D.
18 g
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Solution
N2 + 3H2 → 2NH3. Molar mass of NH3 = 14 + 3 = 17 g.
Correct Answer: A — 28 g
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Q. What is the theoretical yield of Na2SO4 when 10 g of Na reacts with excess sulfuric acid?
A.
20 g
B.
30 g
C.
40 g
D.
50 g
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Solution
10 g of Na = 0.434 moles. 2Na + H2SO4 → Na2SO4 + H2. 0.434 moles of Na2SO4 = 0.434 * 142 g = 61.6 g.
Correct Answer: B — 30 g
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Q. What is the theoretical yield of NaCl when 23 g of Na reacts with Cl2?
A.
58.5 g
B.
23 g
C.
46 g
D.
69 g
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Solution
23 g of Na = 1 mole. 1 mole of Na produces 1 mole of NaCl = 58.5 g.
Correct Answer: A — 58.5 g
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Q. What is the theoretical yield of NaCl when 23 g of Na reacts with excess Cl2?
A.
58.5 g
B.
23 g
C.
46 g
D.
11.5 g
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Solution
23 g of Na = 1 mole. 1 mole of Na produces 1 mole of NaCl = 58.5 g.
Correct Answer: A — 58.5 g
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Q. What is the total number of moles of gas produced when 1 mole of CaCO3 decomposes?
A.
1 mole
B.
2 moles
C.
3 moles
D.
0 moles
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Solution
The decomposition of CaCO3 produces CaO and CO2: CaCO3 → CaO + CO2. This results in 1 mole of gas (CO2) being produced.
Correct Answer: B — 2 moles
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Q. What is the total number of moles of gas produced when 1 mole of CaCO3 decomposes to form CaO and CO2?
A.
0.5 moles
B.
1 mole
C.
2 moles
D.
3 moles
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Solution
The decomposition reaction is CaCO3 → CaO + CO2. This produces 1 mole of CaO and 1 mole of CO2, totaling 2 moles of gas.
Correct Answer: C — 2 moles
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Q. What is the volume of 1 mole of gas at STP?
A.
22.4 L
B.
24 L
C.
20 L
D.
18 L
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Solution
At STP, 1 mole of gas occupies 22.4 liters.
Correct Answer: A — 22.4 L
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Q. What is the volume of CO2 produced at STP when 2 moles of C2H5OH are completely combusted?
A.
22.4 L
B.
44.8 L
C.
67.2 L
D.
89.6 L
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Solution
C2H5OH + 3O2 → 2CO2 + 3H2O. 2 moles of C2H5OH produce 4 moles of CO2. Volume = 4 * 22.4 L = 89.6 L.
Correct Answer: B — 44.8 L
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Q. What volume of 0.5 M HCl is required to completely react with 0.1 moles of Na2CO3?
A.
200 mL
B.
400 mL
C.
100 mL
D.
300 mL
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Solution
The reaction is Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2. 0.1 moles of Na2CO3 requires 0.2 moles of HCl. Volume = moles / concentration = 0.2 moles / 0.5 M = 0.4 L or 400 mL.
Correct Answer: B — 400 mL
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Q. What volume of 0.5 M NaCl solution contains 1 mole of NaCl?
A.
1 L
B.
2 L
C.
0.5 L
D.
0.25 L
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Solution
Using the formula Molarity (M) = moles/volume (L), we have 0.5 M = 1 mole/volume. Therefore, volume = 1 mole / 0.5 M = 2 L.
Correct Answer: A — 1 L
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Q. What volume of 0.5 M NaOH solution contains 1 mole of NaOH?
A.
1 L
B.
2 L
C.
0.5 L
D.
0.25 L
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Solution
Using the formula Molarity (M) = moles/volume (L), we rearrange to find volume = moles/Molarity. Thus, volume = 1 mole / 0.5 M = 2 L.
Correct Answer: A — 1 L
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Q. What volume of 1 M NaOH solution is required to completely neutralize 0.5 moles of HCl?
A.
0.5 L
B.
1 L
C.
0.25 L
D.
2 L
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Solution
The reaction between NaOH and HCl is 1:1. Therefore, to neutralize 0.5 moles of HCl, 0.5 moles of NaOH are required, which corresponds to 0.5 L of 1 M NaOH solution.
Correct Answer: A — 0.5 L
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