Concept explainers
(a)
Interpretation : The number of moles of
Concept Introduction : A
The moles and grams of reactant and product can be calculated with the help of mole concept.
(b)
Interpretation : The mass of
Concept Introduction : A chemical reaction involves the formation of some new product molecules with the help of some reactant molecules either by bond making or bond breaking.
The moles and grams of reactant and product can be calculated with the help of mole concept.
(c)
Interpretation : The mass of water produced when 12.2 g of
Concept Introduction : A chemical reaction involves the formation of some new product molecules with the help of some reactant molecules either by bond making or bond breaking.
The moles and grams of reactant and product can be calculated with the help of mole concept.
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Basic Chemistry
- The burning of iron pyrites (FeS.) in air may be expressed by the following reaction: Fes2 + 02 -> Fe203 + SO2 а. What mass of iron pyrite must be burned in air to produce 400.0g of ferric oxide? (8) b. What mass of oxygen will be consumed? ( C. How many molecules of sulfur dioxide will be produced ?arrow_forward(5.8)Which of the following reactions will form a gaseous product? O H₂CO3(aq) + Pb(NO3)2(aq) O NaOH(aq) + HNO3(aq) O None of these O Na₂SO3(aq) + H₂SO4(aq) ◄ Previousarrow_forwardQuestion 16 of 40 Balance the following chemical equation (if necessary): C3H,O2(g) + O2(g) → H2O(g) + CO2(g) H2O (g) + CO2 (g) 3C2 2- Reset 1. 2. 4 6. 8. 9. ) (s) (1) (g) (aq) LO 3.arrow_forward
- 9.24 For each of the following reactions, 20.0 g of each reactant is present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced. 2Al2O3(s) (Al2O3) 109sh HOUT a. 4Al(s) + 302(g) b. 3NO2(g) + H2O(l) → c. C₂HO(l) + 302(g) 2HNO3(aq) + NO(g) 2CO2(g) + 3H2O(g) (HNO3) (H₂O)arrow_forwardIn an experiment, 7.84 g of sulphuric acid reacts with potassium carbonate. H2SO4 + K2CO3 —> K2SO4 + H2O + CO2 Calculate: the mass of potassium carbonate consumed (11.0g)arrow_forward9:55 ull LTE Question 4 of 15 Submit Determine the mass in grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C4H10(g) + 13 O2(g) → CO2(g) + 10 H20(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.0374 2 mol C4H10 1 mol CO2 8.70 44.01 g H20 2.18 4.35 g O2 18.02 208.00 g CH10 126 13 mol H20 10 6.022 x 1023 mol O2 58.14 g CO2 Tap here or pull up for additional resourcesarrow_forward
- Barium Hydroxide has a solubility of 4.68 g Ba(OH)2 in 100. g H2O at 25°C. Determine if each of the following solutions will be saturated or unsaturated at 25°C: (9.3) a) adding 32 g of Ba(OH)2 to 990 g of H2O b) adding 7.0 g of Ba(OH)2 to 125 g of H2O c) adding 22 g of Ba(OH)2 to 350. g of H2Oarrow_forward(4.3: Similar to Conceptual Connection) How many moles of O₂(g) are required to react with 5.38 moles of C4H10(g) according to the following reaction? 2C4010(g) + 1302(g) --> 8CO2(g) + 10H₂O(g) O 16.1 mol O 29.6 mol O 69.9 mol 35.0 molarrow_forward(LO 7.1.1, 7.1.2, 7.2.1, 7.2.2) A small home might use about 6.50 moles of methane, CH4, per day in moderately cold weather for heating. How many moles of water will be produced when combusting 6.50 moles of methane? CH4 + CO₂ + 2.17 3.25 4.33 6.5 9.75 13.0 19.5 0₂ → 111- H₂O (unbalanced)arrow_forward
- 8. 9. 10. 4 Fe + 3 0₂ → 2 Fe₂O3 If you have 43 grams of oxygen, how many mols of iron(III) oxide will be formed? If you have 7.5 mol of iron, how many mols of oxygen would be required? If you have 125 g of iron, how many grams of iron(III) oxide will be formed? was per the an de and the red nox 91arrow_forward6.(0-2) Black powder was invented in China in the 9th century. It was used as an explosive with propelling properties. Today it is used in fireworks, model rocket engines, and replica black powder weapons. Black powder consists of potassium nitrate (potassium nitrate, KN03), charcoal and sulfur. A variety of chemical reactions take place when this mixture is exploded. One of these is shown below. 2KNO, +S+ 30 → K, S+N, ↑+3C0, 1 Knowing that carbon makes up 15% of the black powder, calculate the total volume of gases (under normal conditions) released when 0.1 kg of black powder explodes. Assume that only the chemical reaction given above occurs.arrow_forwardHomework Problems 4.1 Calculate the number of moles in a 5.00-g sample of each of the following: a. Caffeine (C8H10N402) b. Aspirin (C9H8O4) c. PenicillinV (C16H18N2O5S) 4.2 Balance the following equations: a. Cl₂O7 + H₂O ->>> HC104 b. Fe2(CO3)3 Fe2O3 + CO₂ c. H3PO4 + Mn(OH)2 - Mn3(PO4)2+ H₂O d. P₂H4 → PH3 + P4 e. SO₂Cl2 + HI→ H₂S + H₂O + HC1 + 1₂ 4.3 Write the formula equation, total ionic and net ionic equations for each of the following: a. The reaction of Pb(NO3)2 and LiCl. b. The reaction of ZnSO4 and KOH. 4.4 In the following redox reactions, identify what is oxidized and what is reduced: a. Zn(s) + 2Ag (aq) → Zn²+(aq) + 2Ag(s) - b. Sn²+ (aq) + 2Ce+(aq) c. 2Au(s) + 6H*(aq) d. 4Co(s) + 302(g) e. 2CO(g) + O2(g) → → Sn(aq) + 2Ce³+ (aq) 3+ 2Au³+ (aq) + 3H₂(g) 2C0203(s) 2CO2(g) 4-24arrow_forward
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