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iren [92.7K]
2 years ago
11

Ethanol is highly toxic if it is consumed in large quantities. Although it is the second least toxic of the five alcohols discus

sed in this case, the ingestion of large quantities of ethanol is not safe. One serious problem with ethanol consumption is how the quantity is conveyed to the consumer. For example, American malt liquor can be sold in 23.5 fl. oz. (695 mL) cans and is 12% volume per volume (v/v) ethanol. Although these cans are labeled as containing multiple servings, many young people consider one can to be a single serving. Drinking two cans of this beverage can result in an accidental overdose of ethanol. Two cans may not seem like much until you do the math. In the previous question, you determined that the total volume of pure ethanol in a 695 mL can of American malt liquor is 83.4 mL. To better understand its significance, consider how this volume of ethanol compares with other alcoholic beverages. Calculate the total volume of ethanol in a standard 25.4 fl. oz (750 mL) bottle of liquor (e.g., whiskey, vodka, rum, etc.), which is typically 40% (v/v) ethanol. Enter your answer in milliliters. pure ethanol in liquor: mL Now calculate the total volume of ethanol in a typical 12 fl. oz (354.8 mL) can of light beer, which is 4% (v/v) ethanol. Enter your answer in milliliters. pure ethanol in light beer:
Chemistry
1 answer:
Kobotan [32]2 years ago
6 0

A significant MOE exists compared to developmental toxicity effect levels.

Blood alcohol levels from ABHS approximate consumption of non-alcoholic beverages.

No significant risk of developmental toxicity is expected from ABHS use.

Ethanol-based topical antiseptic hand rubs, commonly referred to as alcohol-based hand sanitizers (ABHS), are routinely used as the standard of care to reduce the presence of viable bacteria on the skin and are an important element of infection control procedures in the healthcare industry.

There are no reported indications of safety concerns associated with the use of these products in the workplace. However, the prevalence of such alcohol-based products in healthcare facilities and safety questions raised by the U.S. FDA led us to assess the potential for developmental toxicity under relevant product-use scenarios.

Estimates from a physiologically based pharmacokinetic modeling approach suggest that occupational use of alcohol-based topical antiseptics in the healthcare industry can generate low, detectable concentrations of ethanol in blood.

This unintended systemic dose probably reflects contributions from both dermal absorption and inhalation of the volatilized product.

Learn more about Ethanol at

brainly.com/question/5750283

#SPJ4

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Water is 11.2% by mass hydrogen. How many kilograms of water would contain 5.8 g of hydrogen?
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Which element, under normal circumstances, does not combine chemically with other elements to form compounds?
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A dehydration reaction starting with 3.8 g cyclohexanol produces 2.6 g cyclohexene. Calculate the theoretical yield for this rea
diamong [38]

Answer:

Theoretical yield of C6H10 = 3.2 g.

Explanation:

Defining Theoretical yield as the quantity of product obtained from the complete conversion of the limiting reactant in a chemical reaction. It can be expressed as grams or moles.

Equation of the reaction

C6H11OH --> C6H10 + H2O

Moles of C6H11OH:

Molar mass of C6H110H = (12*6) + (1*12) + 16

= 100 g/mol

Mass of C6H10 = 3.8 g

number of moles = mass/molar mass

=3.8/100

= 0.038 mol.

Using stoichoimetry, 1 moles of C6H110H was dehydrated to form 1 mole of C6H10 and 1 mole of water.

Therefore, 0.038 moles of C6H10 was produced.

Mass of C6H10 = molar mass * number of moles

Molar mass of C6H10 = (12*6) + (1*10)

= 82 g/mol.

Mass = 82 * 0.038

= 3.116 g of C6H10.

Theoretical yield of C6H10 = 3.2 g

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Answer:

ga

Explanation:

beacuse it its the voltage that high

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