a.
To determine:
The main product of the hydration in the given
Concept introduction:
Hydration is a type of addition reaction in which
Some of alcohols that are produced industrially from this type of reaction are ethanol and
b.
To determine:
The main product of the hydration in the given alkene.
Concept introduction:
Hydration is a type of addition reaction in which
Some of alcohols that are produced industrially from this type of reaction are ethanol and
c.
To determine:
The main product of the hydration in the given alkene.
Concept introduction:
Hydration is a type of addition reaction in which
Some of alcohols that are produced industrially from this type of reaction are ethanol and
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General, Organic, and Biological Chemistry (3rd Edition)
- A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardChlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a ClO2 molecule at 25C is 306 m/s. What is the kinetic energy (in joules) of a ClO2 molecule moving at this speed?arrow_forward
- Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.arrow_forwardWould the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.arrow_forwardThe equation for the combustion of 2 mol of butane can be written 2C4H10(g)+O2(g)8CO2(g)+10H2O(g);HO Which of the following produces the least heat? a Burning 1 mol of butane. b Reacting 1 mol of oxygen with excess butane. c Burning enough butane to produce 1 mol of carbon dioxide. d Burning enough butane to produce 1 mol of water. e All of the above reactions (a, b, c, and d) produce the same amount of heat.arrow_forward
- How much would the temperature of 275 g of water increase if 36.5 U of heat were added?arrow_forward2. A 1.07 g sample of sulfur was burned in a bomb calorimeter with calorimeter constant of 2.03 kcal/°C. If the resulting temperature change was 1.17°C, what is the molar heat of combustion for sulfur in kcal/mole? 1.11arrow_forwardFrom the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18 + 25O2 ---> 16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases. How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?arrow_forward
- 3. The heat of the solution of a solid sample was determined using a coffee cup calorimeter that contains 250ml of water initially at 25C. As the sample is dissolved in the water, the temperature of the water decreased to 11C. What is the heat of the solution of the sample? Assume that the density of water is 1.00g/ml and that the coffee cup is a good insulator. Is the process endothermic or exothermic?arrow_forwardCalculate Kpfor the reaction 2NOCl(g) -> 2NO(g) + Cl2(g) at 400°C if Kcat 400°C for this reaction is 2.1 × 10–2.arrow_forwardQuestion 7arrow_forward
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