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omeli [17]
3 years ago
11

Shelby measured the volume of a cylinder and determined it to be 54.5cm3. The teacher told her that she was 4.25% too high in he

r determination of the volume. What is the actual volume of the cylinder ?
Chemistry
1 answer:
FinnZ [79.3K]3 years ago
6 0

Answer:

56.8cm³

Explanation:

Given parameters:

Measured volume = 54.5cm³

Percentage error  = 4.25%

Unknown:

Actual volume of the cylinder = ?

Solution:

The percentage error shows the amount of error introduced into a measurement.

We need to find out this amount of error from the data given.

   Error = Percentage error x measured volume

                       Error = \frac{4.25}{100} x 54.5  = ±2.32cm³

Since the error introduced = 2.32cm³

  Actual volume of cylinder = measured volume ± Error

  Since the percentage error quoted as higher 4.25%;

 Actual volume  = 54.5cm³ + 2.32cm³ = 56.8cm³

       

 

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Explanation:

When fluorine gas reacts with calcium metal at high temperatures then it results into the formation of calcium fluoride.

Since, calcium has 2 extra electrons as its electronic distribution is 2, 8, 8, 2. Whereas each fluorine atom needs one electron to complete its octet.

Therefore, the chemical reaction equation will be as follows.

      Ca(s) + F_{2}(g) \rightarrow CaF_{2}(s)  

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3 years ago
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You start with 1 L of CO2 at standard temperature and pressure in a closed container. If you raise the temperature of the gas, t
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Answer:

Increase

Explanation:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

If the initial temperature and pressure is standard,

Pressure = 1 atm

Temperature = 273.15 K

then we increase the temperature to 400.0 K, The pressure will be,

1 atm / 273.15 K = P₂/400.0K

P₂ = 1 atm × 400.0 K / 273.15 K

P₂ = 400.0 atm. K /273.15 K

P₂ = 1.46 atm

Pressure is also increase from 1 atm to 1.46 atm.

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3 years ago
There is nothing that you can do to conserve energy. True or False
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What are the mole fraction and the mass percent of a solution made by dissolving 0.21 g KBr in 0.355 L water? (d = 1.00 g/mL.) m
IRISSAK [1]

Answer:

Mol fraction H2O = 0.99991

Mol fraction KBr = 0.00009

mass % KBr = 0.059 %

mass % H2O = 99.941 %

Explanation:

Step 1: Data given

Mass of KBr = 0.21 grams

Molar mass KBr = 119 g/mol

Volume of water = 355 mL

Density of water = 1.00 g/mL

Molar mass water = 18.02 g/mol

Step 2: Calculate mass water

Mass water = 355 mL * 1g /mL

Mass water = 355 grams

Step 3: Calculate moles water

Moles water = mass water / molar mass water

Moles water = 355 grams / 18.02 g/mol

Moles water = 19.7 moles

Step 4: Calculate moles KBr

Moles KBr = 0.21 grams / 119 g/mol

Moles KBr = 0.00176 moles

Step 5: Calculate total moles

Total moles = 19.7 moles + 0.00176 moles

Total moles = 19.70176 moles

Step 6: Calculate mol fraction

Mol fraction H2O = 19.7 moles / 19.70176 moles

Mol fraction H2O = 0.99991

Step 7: Calculate mol fraction KBr

Mol fraction KBr = 0.00176 / 19.70176

Mol fraction KBr = 0.00009

Step 6: Calculate mass %

mass % KBR = (0.21 grams / (0.21 + 355) grams) *100%

mass % KBr = 0.059 %

mass % H2O = (355 grams / 355.21 grams) *100%

mass % H2O = 99.941 %

8 0
3 years ago
Give the reason for the following; 1. Iodimetric titrations are usually performed in neutral or mildly alkaline (pH 8) to weakly
Agata [3.3K]

Answer:

Explanation:

blach bal

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3 years ago
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