StudentAidUnit 15: Unit 15: Stoichiometry — Mcqs
10th Class Chemistry · Unit 15: Stoichiometry
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1.Volume occupied by 15 moles of ammonia gas at RTP:
2.How many moles of natural gas CH₄ will be present in a cylinder if its volume is 18 dm³ at RTP?
3.What will the molar concentration of potassium hydroxide solution if 2.0 g of it are dissolved in 100 cm³ of solution?
4.What will be the mass of NaCℓ needed to make up 15 dm³ of its solution with a concentration of 0.7 g/dm³?
5.Find out the concentration of H₂SO₄ in mol/dm³ if its 10 cm³ react with 20 cm³ of NaOH solution having concentration 0.1 mol/dm³.
6.If the molar mass of a compound is 178 g/mol and its empirical formula is C₃H₅O₃. What is its molecular formula?
7.When natural gas burns in air, which component is the limiting reactant?
8.If the actual yield of a compound is 0.198 g while the theoretical yield is 0.217 g. What will be the percentage yield?
Molar Volume
9.The room temperature and pressure (RTP) is:
10.Calculate the number of moles of CH₄ gas, when its volume is 5dm³ at RTP:
11.7.5 moles of the gas contain ________ dm³ of volume at RTP.
12.Calculate the volume of CO₂ at RTP when its mass is 88g.
Concentration of a Solution
13.The measure of amount of solute that has been dissolved in a given amount of solution is __________.
14.Calculate the mass of sodium carbonate (Na₂CO₃) in a solution of volume 2dm³ having concentration of 0.5g/dm³.
Calculate the Concentration in Titration using empirical formula
15.Calculate concentration of a solution in g/dm³ which contains 0.2g of calcium acetate dissolved in 4.5dm³ of solution:
16.100cm³ of hydrochloric acid contains 0.4g of dissolved hydrogen chloride. Calculate the concentration of the acid in g/dm³:
17.Molar concentration and ________ both refer to the concentration of a solute in a solution.
18.What is the mass of potassium fluoride in grams dissolved in 0.1 dm³ of solution having concentration of 0.001 g/dm³?
19.The concentration of a solution can be determined by titrating it with a solution of __________ till the end point reached.
20.In titration __________ will change its colour to show and point.
21.Stoichiometry is essential for __________ chemical reactions in many industries.
Percentage Composition by Mass, Empirical and Molecular Formula
22.Percentage composition of a compound is the percentage mass of each __________ present in the compound.
23.The percentage of H-atom in H₂O is:
24.To determine molecular and empirical formula, __________ is useful concept.
25.The percentage of calcium (Ca) in CaCO₃:
26.The percentage of an element is type analysis:
27.What is the percentage of C in CH₄?
28.Calculate percentage of chloride (Cl⁻¹) ions in CaCℓ₂:
Empirical formula
29.Which of the following pair is correct empirical formula and atomic ratio of H₂SO₄?
30.All __________ compounds are represented only by their empirical formula:
31.The empirical formula of a gas ethyne (C₂H₂) used in cutting and welding of metals is:
32.Empirical formula shows the __________ number ratio of atoms in a compound:
33.Number of steps used to calculate empirical formula of a compound are:
34.The atomic ratio in empirical formula can be found by dividing the number of moles of each element by the
35.The empirical formula of acetic acid C₂H₄O₂ is:
36.Which one of the following is not an empirical formula?
Molecular formula
37.Which one of the following compound will have same molecular and empirical formula?
38.__________ is used to determine the optimal dosages of medicines for patients based on their weight and age etc.
39."n" is a number find by dividing molecular mass with __________.
40.Which one of the following is the molecular formula of ethylene?
Calculations Based On Chemical Equation
41.A complete balanced chemical equation tells about __________ between reactants and products:
42.2H₂₍ₘ₎ + O₂₍ₘ₎ -----→ 2H₂O₍ₘ₎, when 64g of O₂ reacts completely with hydrogen. How many grams of H₂O will produced?
43.NaOH + HCℓ -----→ NaCℓ + H₂O, the mole ratio between reactants in this reaction is:
44.In the decomposition of calcium carbonate, when 200g of calcium carbonate Ca(CO₃) is heated, the mass of CaO will be: CaCO₃₍ₛ₎ ----→ CaO₍ₛ₎ + CO₂₍ₘ₎
Limiting Reactant
45.In a chemical reaction, the reactant which consumed earlier is:
46.When 80g of H₂ and 32g of O₂ reacted, the limiting reactant will be: 2H₂ + O₂ -----→ 2H₂O
47.Number of steps to identify limiting reactant is:
48.The reactant that controls the amount of product formed in a chemical reaction is:
Yield
49.The amount of product obtained when chemical reaction is performed called:
50.To check efficiency of reaction. __________ is calculated:
Percentage Purity
51.The unit of percentage purity is:
52.Percentage purity of compound indicates the amount of __________ present in an impure sample: