Q. No.The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber's process is:
1. 40
2. 10
3. 20
4. 30
Subtopic: Equation Based Problem |
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NEET - 2019
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Consider the following combustion reaction:
\(\mathrm{CH}_4+\mathrm{O}_2 \longrightarrow \mathrm{CO}_2+\mathrm{H}_2 \mathrm{O}\)
How many moles of methane (\(\mathrm{CH_4}\)) will be required for the formation of 11 g of carbon dioxide (\(\mathrm{CO_2}\))?
\(\mathrm{CH}_4+\mathrm{O}_2 \longrightarrow \mathrm{CO}_2+\mathrm{H}_2 \mathrm{O}\)
How many moles of methane (\(\mathrm{CH_4}\)) will be required for the formation of 11 g of carbon dioxide (\(\mathrm{CO_2}\))?
| 1. | 0.25 | 2. | 0.62 |
| 3. | 0.17 | 4. | 1.23 |
Subtopic: Equation Based Problem |
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The following reaction is given for reference:
\(2 \mathrm{KI}+\mathrm{HgI}_2 \rightarrow \mathrm{K}_2 \mathrm{HgI}_4\)
The number of moles of KI required to produce 0.4 moles of K2HgI4 is:
1. 0.4
2. 0.8
3. 3.2
4. 1.6
\(2 \mathrm{KI}+\mathrm{HgI}_2 \rightarrow \mathrm{K}_2 \mathrm{HgI}_4\)
The number of moles of KI required to produce 0.4 moles of K2HgI4 is:
1. 0.4
2. 0.8
3. 3.2
4. 1.6
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Calculate mass of CH4 consumed for the formation of 22 g CO2.
CH4 + 2O2 → CO2 + 2H2O
1. 8
2. 1
3. 9
4. 7
CH4 + 2O2 → CO2 + 2H2O
1. 8
2. 1
3. 9
4. 7
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During the reaction of 32.65 g of zinc with HCl, what is the volume of hydrogen gas liberated at STP?
(atomic mass of Zn=65.3u)
1. 20 L
2. 15.23 L
3. 11.2 L
4. 25.5 L
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What is the volume of CO₂ produced from the complete decomposition of 20 g of CaCO₃ at STP?
1. 2.24 litre
2. 4.48 litre
3. 20 litre
4. 22.4 litre
1. 2.24 litre
2. 4.48 litre
3. 20 litre
4. 22.4 litre
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At 120 ºC and 1 atm pressure, 1.00 L of methane reacts completely with excess oxygen to form carbon dioxide and water.
The volumes of the two products at this pressure and temperature are:
1. 1.00 L CO2 and 2.00 L H2O.
2. 1.00 L CO2 and 4.00 L H2O.
3. 2.00 L CO2 and 2.00 L H2O.
4. 2.00 L CO2 and 4.00 L H2O.
The volumes of the two products at this pressure and temperature are:
1. 1.00 L CO2 and 2.00 L H2O.
2. 1.00 L CO2 and 4.00 L H2O.
3. 2.00 L CO2 and 2.00 L H2O.
4. 2.00 L CO2 and 4.00 L H2O.
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The number of moles of methane are required to produce 22g CO2(g) after complete combustion is:
1. 1 mole
2. 0.5 mole
3. 1.5 mole
4. 2 mole
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Barium reacts with water according to the following reaction:
\(\mathrm{Ba}(\mathrm{s})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{Ba}(\mathrm{OH})_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})\)
What volume of hydrogen gas, at standard temperature and pressure (STP), is produced from 0.400 mol of barium?
\(\mathrm{Ba}(\mathrm{s})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{Ba}(\mathrm{OH})_2(\mathrm{aq})+\mathrm{H}_2(\mathrm{~g})\)
What volume of hydrogen gas, at standard temperature and pressure (STP), is produced from 0.400 mol of barium?
| 1. | 8.96 L | 2. | 5.60 L |
| 3. | 4.48 L | 4. | 3.36 L |
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Upon strong heating, what is the weight of the residue produced by 2.76 gram silver carbonate? Consider the following reaction for reference:
\(\mathrm{Ag_2CO_3 \rightarrow 2Ag+CO_2+{{1/2}}~O_2}\)
1. \(2.16~g\)
2. \(2.48~g\)
3. \(2.32~g\)
4. \(2.64~g\)
\(\mathrm{Ag_2CO_3 \rightarrow 2Ag+CO_2+{{1/2}}~O_2}\)
1. \(2.16~g\)
2. \(2.48~g\)
3. \(2.32~g\)
4. \(2.64~g\)
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