Concept explainers
A mixture of tetraphosphorus trisulfide and powdered glass is in the white tip of strike-anywhere matches. The
The tips of strike-anywhere matches contain tetraphosphorus trisulfide,
which reacts with the oxygen in the air in an exothermic change to inititae
the burning reaction.
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Chapter 10 Solutions
Introductory Chemistry: An Active Learning Approach
- The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)arrow_forwardThe reaction of iron metal and chlorine gas to give iron(III) chloride is illustrated below. (a) Write the balanced chemical equation for the reaction. (b) Beginning with 10.0 g of iron, what mass of Cl2, in grams, is required for complete reaction? What mass of FeCl3 can be produced? (c) If only 18.5 g of FeCl3 is obtained from 10.0 g of iron and excess Cl2, what is the percent yield? (d) If 10.0 g each of iron and chlorine are combined, what is the theoretical yield of iron(III) chloride?arrow_forward4.84 Aluminum chloride (AlCl3) is used as a catalyst in the production of polyisobutylene, which is used in automobile tires. Scrap aluminum metal reacts with chlorine gas (Cl2) to produce AlCl3. Suppose that 2.70 g of Al and 7.10 g of Cl2 are mixed. What is the maximum mass of AlCl3 that could be formed?arrow_forward
- Boron forms an extensive series of compounds with hydrogen, all with the general formula BxHy. To analyze one of these compounds, you burn it in air and isolate the boron in the form of B2O3 and the hydrogen in the form of water. You find that 0.1482 g BxHy gives 0.4221 g B2O3 when burned in excess O2. Determine the empirical I formula of BxHy.arrow_forwardBoth water and sulfur dioxide are products from the reaction of sulfuric acid (H2SO4) with copper metal, asshown by the equation 2H2SO4 + Cu SO2 + 2H2O + CuSO4 How many grams of H2O will be produced at the same time that 10.0 g of SO2 is produced?arrow_forwardWhen dinitrogen pentoxide, N2O5, a white solid, is heated, it decomposes to nitrogen dioxide and oxygen. 2N2O5(s)4NO2(g)+O2(g) If a sample of N2O5 produces 1.381 g O2, how many grams of NO2 are formed?arrow_forward
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