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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

An “ice calorimeter” can be used to determine the specific heat capacity of a metal. A piece of hot metal is dropped onto a weighed quantity of ice. The energy transferred from the metal to the
Enthalpy changes for the following reactions can be determined experimentally: Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that
A 9.36-g piece of platinum was heated to 98.6°C in a boiling water bath and then dropped onto ice. (See Study Question 47.) When the metal’s temperature had dropped to 0.0°C, it was found that
You wish to know the enthalpy change for the formation of liquid PCl3 from the elements. The enthalpy change for the formation of PCl5 from the elements can be determined experimentally, as can the
Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:(a) 1.0 g of white phosphorus burns, forming P4O10(s)(b) 0.20 mol of NO(g) decomposes to N2(g) and
What does the term standard state mean? What are the standard states of the following substances at 298 K: H2O, NaCl, Hg, CH4?
Which evolves more energy on cooling from 50°C to 10°C: 50.0 g of water or 100. g of ethanol (Cethanol = 2.46 J/g ∙ K)?
You determine that 187 J of energy as heat is required to raise the temperature of 93.45 g of silver from 18.5°C to 27.0°C. What is the specific heat capacity of silver?
The standard molar enthalpy of formation of diborane, B2H6(g), cannot be determined directly because the compound cannot be prepared by the reaction of boron and hydrogen. It can be calculated from
Suppose that only two 45-g ice cubes had been added to your glass containing 5.00 × 102 mL of tea. When thermal equilibrium is reached, all of the ice will have melted, and the temperature of the
You take a diet cola from the refrigerator and pour 240 mL of it into a glass. The temperature of the beverage is 10.5°C. You then add one ice cube (45 g) at 0°C. Which of the following describes
When heated to a high temperature, coke (mainly carbon, obtained by heating coal in the absence of air) and steam produce a mixture called water gas, which can be used as a fuel or as a starting
Camping stoves are fueled by propane (C3H8), butane [C4H10(g), ∆fH° = −127.1 kJ/mol], gasoline, or ethanol (C2H5OH). Calculate the enthalpy of combustion per gram of each of these fuels. [Assume
Hydrazine and 1,1-dimethylhydrazine both react spontaneously with O2 and can be used as rocket fuels.The molar enthalpy of formation of N2H4(ℓ) is +50.6 kJ/mol, and that of N2H2(CH3)2(ℓ) is +48.9
(a) Calculate the enthalpy change, ∆rH°, for the formation of 1.00 mol of strontium carbonate (the material that gives the red color in fireworks) from its elementsThe experimental information
Methanol, CH3OH, a compound that can be made relatively inexpensively from coal, is a promising substitute for gasoline. The alcohol has a smaller energy content than gasoline, but, with its higher
Chloroform, CHCl3, is formed from methane and chlorine in the following reaction.Calculate ∆rH°, the enthalpy change for this reaction, using the enthalpies of formation of CO2(g), H2O(ℓ), and
Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of coke or coal) with steam at high temperatures. (See Study Question 83.Not all of the carbon
You drink 350 mL of diet soda that is at a temperature of 5°C.(a) How much energy will your body expend to raise the temperature of this liquid to body temperature (37°C)? Assume that the density
Using standard enthalpies of formation, verify that 2680 kJ of energy is released in combustion of 100.0 g of ethanol. C₂H5OH() + 3 O₂(g) 2 CO₂(g) + 3 H₂O(g)
According to the Nutrient Data Laboratory website (www.ars.usda.gov/ba/bhnrc/ndl), corn oil contains 3766 kJ of energy per 100. g serving. (a) What is the energy content of 100. g of corn oil in
A piece of lead with a mass of 27.3 g was heated to 98.90°C and then dropped into 15.0 g of water at 22.50°C. The final temperature was 26.32°C. Calculate the specific heat capacity of lead from
The value of ∆U for the decomposition of 7.647 g of ammonium nitrate can be measured in a bomb calorimeter. The reaction that occurs is The temperature of the calorimeter, which contains 415 g of
A 192-g piece of copper is heated to 100.0°C in a boiling water bath and then dropped into a beaker containing 751 g of water (density = 1.00 g/cm3) at 4.0°C. What was the final temperature of the
The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called “Heater Meals.” Just pour water into the heater unit, wait a few
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction isThe bomb had a heat capacity of 550 J/K, and the calorimeter contained 650 g of water.
You want to determine the value for the enthalpy of formation of CaSO4(s), but the reaction cannot be done directly.You know, however, that(a) Both calcium and sulfur react with oxygen to produce
Without doing calculations, decide whether each of the following is exo- or endothermic. (a) The combustion of natural gas (b) The decomposition of glucose, C6H12O6, to carbon and water
Which of the following are state functions? (a) The volume of a balloon (b) The time it takes to drive from your home to your college or university(c) The temperature of the water in a coffee
Prepare a graph of specific heat capacities for metals versus their atomic weights. Combine the data in Figure 5.4 and the values in the following table. What is the relationship between specific
Observe the molar heat capacity values for the metals in Figure 5.4. What observation can you make about these values—specifically, are they widely different or very similar? Using this
You are attending summer school and living in a very old dormitory. The day is oppressively hot, there is no air conditioner, and you can’t open the windows of your room. There is a refrigerator in
You want to heat the air in your house with natural gas (CH4). Assume your house has 275 m2 (about 2800 ft2) of floor area and that the ceilings are 2.50 m from the floors. The air in the house has a
Water can be decomposed to its elements, H2 and O2, using electrical energy or in a series of chemical reactions. The following sequence of reactions is one possibility:(a) Show that the net result
Write balanced chemical equations for the following reactions:(a) Production of ammonia, NH3(g), by combining N2(g) and H2(g)(b) Production of methanol, CH3OH(ℓ) by combining H2(g) and CO(g)(c)
Balance the following equations: (a) Cr(s) + O2(g) n Cr2O3(s)(b) Cu2S(s) + O2(g) n Cu(s) + SO2(g)(c) C6H5CH3(ℓ)+ O2(g) n H2O(ℓ) + CO2(g)Data given in Example 3.1 EXAMPLE 3.1 Balancing an
Balance the following equations: Data given in Example 3.1 (a) Cr(s) + Cl₂(g) → CrCl3(s) (b) SiO₂ (s) + C(s) → Si(s) + CO(g) (c) Fe(s) + H₂O(g) → Fe3O4(s) + H₂(g)
Balance the following equations, and name each reactant and product: Data given in Example 3.1 (a) FeO3(s) + Mg(s) MgO(s) + Fe(s) (b) AlCl3(s) + NaOH(aq) AI(OH)3 (s) + NaCl(aq) (c) NaNO3(s) +
Balance the following equations, and name each reactant and product:Data given in Example 3.1 (a) SF4(g) + H₂O(l) → SO₂(g) + HF(e) (b) NH3(aq) + O₂(aq) → NO(g) + H₂O(l) (c) BF3(g) +
Write balanced chemical equations for the following reactions.(a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction).(b) The reaction of
Carry out the following operations. Provide the answer with the correct number of significant figures.(a). (1.52)(6.21 × 10−3) (b). (6.217 × 103)−(5.23 × 102) (c). (6.217 × 103) ÷ (5.23 ×
The equation for the oxidation of phosphorus in air is Identify the reactants and products and the stoichiometric coefficients. To what do the designations s and g refer? P4(s) + 5 O₂(g) →
Strontium has four stable isotopes. Strontium-84 has a very low natural abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Knowing that the atomic weight of strontium is 87.62, which of
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
The equation for the reaction of phosphorus and chlorine is If you use 8000 molecules of P4 in this reaction how many molecules of Cl2 are required to consume the P4 completely? P4(s) + 6 Cl₂(g)
Which of the following compounds has the highest mass percent of chlorine?(a) BCl3(b) AsCl3(c) GaCl3(d) AlCl3(e) PCl3
The equation for the reaction of aluminum and bromine is If you use 6.0 × 1023 molecules of Br2 in a reaction how many atoms of Al will be consumed? 2 Al(s) + 3 Br₂(l) → Al₂Bro(s)
Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams of oxygen were required in this reaction? P4(s) + 6 Cl₂(g) 4 PCL3 (1) reactants product
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction? P4(s) + 6 Cl₂(g) 4 PCL3 (1) reactants product
Equal amounts of two acids—HCl and HCO2H (formic acid)—are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the
Identify each of the following statements as either true or false.(a) At equilibrium the rates of the forward and reverse reactions are equal.(b) When a reaction reaches equilibrium the forward and
Identify each of the following statements as either true or false.(a) All chemical reactions are product-favored at equilibrium.(b) There is no observable change in a chemical system at
Two aqueous solutions were prepared, one containing 0.10 mol of boric acid (H3BO3) in 200 mL and the second containing 0.10 mol phosphoric acid (H3PO4) in 200 mL. Both were weak conductors of
What is an electrolyte? How can you differentiate experimentally between a weak electrolyte and a strong electrolyte? Give an example of each.
Name and give the formulas of two acids that are strong electrolytes and one acid that is a weak electrolyte. Name and give formulas of two bases that are strong electrolytes and one base that is a
Which compound or compounds in each of the following groups is (are) soluble in water? (a) CuO, CuCl2, FeCO3(b) AgI, Ag3PO4, AgNO3(c) K2CO3, KI, KMnO4
Which compound or compounds in each of the following groups is (are) soluble in water? (a) BaSO4, Ba(NO3)2, BaCO3(b) Na2SO4, NaClO4, NaCH3CO2(c) AgBr, KBr, Al2Br6
The following compounds are water-soluble. What ions are produced by each compound in aqueous solution? (a) KOH(b) K2SO4(c) LiNO3(d) (NH4)2SO4
The following compounds are water-soluble. What ions are produced by each compound in aqueous solution? (a) KI(b) Mg(CH3CO2)2(c) K2HPO4(d) NaCN
Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species (s, ℓ, aq, or g). CdCl₂ + NaOH → Cd(OH)₂ + NaCl
Decide whether each of the following is watersoluble. If soluble, tell what ions are produced when the compound dissolves in water. (a) Na2CO3(b) CuSO4(c) NiS(d) BaBr2
Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species (s, ℓ, aq, or g). Ni(NO3)2 + Na₂CO3 → NICO3 + NaNO3
Decide whether each of the following is watersoluble. If soluble, tell what ions are produced when the compound dissolves in water.(a) NiCl2(b) Cr(NO3)3(c) Pb(NO3)2(d) BaSO4
Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation. (a) NiCl₂(aq) + (NH4)₂S(aq) → (b) Mn(NO3)2(aq) + Na3PO4(aq) →
Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation. (a) Pb(NO3)2(aq) (b) Ca(NO3)2(aq) (c) Ca(NO3)2(aq) + KBr(aq) → + KF(aq) → +
Oxalic acid, H2C2O4, which is found in certain plants, can provide two hydronium ions in water. Write balanced equations (like those for sulfuric acid on page 142) to show how oxalic acid can supply
Phosphoric acid can supply one, two, or three H3O+ ions in aqueous solution. Write balanced equations (like those for sulfuric acid on page 142) to show this successive loss of hydrogen ions.Data
Write a balanced equation for the ionization of nitric acid in water.
Write a balanced equation for the ionization of perchloric acid in water.
Complete and balance the equations for the following acid–base reactions. Name the reactants and products. (a) CH3CO₂H(aq) + Mg(OH)₂(s) → (b) HClO4(aq) + NH3(aq) →
Write a balanced equation for reaction of the basic oxide, magnesium oxide, with water.
Complete and balance the equations for the following acid–base reactions. Name the reactants and products. (a) H3PO4(aq) + KOH(aq) → (b) H₂C₂O4(aq) + Ca(OH)₂(s) → (H₂C₂O4 is oxalic
Write a balanced equation for the reaction of sulfur trioxide gas with water.
Write a balanced equation for the reaction of barium hydroxide with nitric acid.
Write a balanced equation for the reaction of aluminum hydroxide with sulfuric acid.
Write an equation that describes the equilibrium that exists when nitric acid dissolves in water. Identify each of the four species in solution as either Brønsted acids or Brønsted bases. Does the
Balance the following equations, and then write the net ionic equation. (a) (NH4)2CO3(aq) + Cu(NO3)2(aq) → CuCO3(s) + NH4NO3(aq) (b) Pb(OH)₂(s) + HCl(aq) → PbCl₂(s) + H₂O(l) (c) BaCO3(s)
Write an equation that describes the equilibrium that exists when the weak acid benzoic acid (C6H5CO2H) dissolves in water. Identify each of the four species in solution as either Brønsted acids or
Balance the following equations, and then write the net ionic equation: (a) Zn(s) + HCl(aq) → H₂(g) + ZnCl₂(aq) (b) Mg(OH)2(s) + HCl(aq) → MgCl₂(aq) + H₂O(l) (c) HNO3(aq) + CaCO3(s)
Write two chemical equations, one that shows H2O reacting (with HBr) as a Brønsted base and a second that shows H2O reacting (with NH3) as a Brønsted acid.
Write two chemical equations, one in which H2PO4− is a Brønsted acid (in reaction with the carbonate ion, CO32−), and a second in which HPO42− is a Brønsted base (in reaction with acetic
Balance the following equations, and then write the net ionic equation. Show states for all reactants and products (s, ℓ, g, aq).(a) The reaction of silver nitrate and potassium iodide to give
Balance each of the following equations, and then write the net ionic equation. Show states for all reactants and products (s, ℓ, g, aq). (a) The reaction of sodium hydroxide and iron(II) chloride
Write balanced net ionic equations for the following reactions:(a) The reaction of nitrous acid (a weak acid) and sodium hydroxide in aqueous solution(b) The reaction of calcium hydroxide and
The mineral rhodochrosite is manganese(II) carbonate. Write an overall, balanced equation for the reaction of the mineral with hydrochloric acid, and name the products. ⒸCengage Learning/Charles D.
Write balanced net ionic equations for the following reactions:(a) The reaction of aqueous solutions of silver nitrate and sodium iodide(b) The reaction of aqueous solutions of barium chloride and
Siderite is a mineral consisting largely of iron(II) carbonate. Write an overall, balanced equation for its reaction with nitric acid, and name the products.
Write an overall, balanced equation for the reaction of (NH4)2S with HBr, and name the reactants and products.
Write an overall, balanced equation for the reaction of Na2SO3 with CH3CO2H, and name the reactants and products.
Determine the oxidation number of each element in the following ions or compounds.(a) BrO3−(b) C2O42−(c) F−(d) CaH2(e) H4SiO4(f) HSO4−
Determine the oxidation number of each element in the following ions or compounds.(a) PF6−(b) H2AsO4−(c) UO2+(d) N2O5(e) POCl3(f) XeO42−
Which two of the following reactions are oxidation–reduction reactions? Explain your answer in each case. Classify the remaining reaction. (a) Zn(s) + 2NO3- (aq) + 4 H₂O+ (aq) → Zn²+ (aq) + 2
For each reaction, write an overall, balanced equation and the net ionic equation.(a) The reaction of aqueous lead(II) nitrate and aqueous potassium hydroxide(b) The reaction of aqueous copper(II)
In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent. 2+ (a) Cr₂O₂² (aq) + 3 Sn²+ (aq) + 14 H3O+ (aq) → 2
Balance the following equations, and then classify each as a precipitation, acid–base, or gas-forming reaction. (a) Ba(OH)₂(aq) + HCl(aq) → BaCl,(aq) + H,O(l) (b) HNO3(aq) + COCO3(s)
Balance the following equations, and then classify each as a precipitation, acid–base, or gas-forming reaction. (a) K₂CO3(aq) + Cu(NO3)2(aq) → CuCO3(s) + KNO3(aq) (b) Pb(NO3)2(aq) + HCl(aq)
Which two of the following reactions are oxidation– reduction reactions? Explain your answer briefly. Classify the remaining reaction. (a) CdCl₂(aq) + Na₂S(aq) → CdS(s) + 2 NaCl(aq) (b) 2
In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent. (a) C₂H4(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(l) (b)
Balance the following equations: (a) For the synthesis of urea, a common fertilizer(b) For the reactions used to make uranium(VI) fluoride for the enrichment of natural uranium (c) For the reaction
Balance the following equations:(a) For the reaction to produce “superphosphate” fertilizer(b) For the reaction to produce diborane, B2H6(c) For the reaction to produce tungsten metal from

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