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vagabundo [1.1K]
3 years ago
7

Moby eats three-sixths of a pizza. Which fraction is equivalent to three-sixths?​

Chemistry
1 answer:
katen-ka-za [31]3 years ago
4 0

Answer:

1/2

Explanation:

Half of 6 is 3 so therefore it is a half.

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(Science)<br> why is the 10g of shampoo is more dense than the 10kg of the same shampoo?
igor_vitrenko [27]
Grams (g) is much lighter than kilograms (kg)
6 0
3 years ago
Identify the major ionic species present in an aqueous solution of nh4clo4.
elena-s [515]
7 strong acids are strong electrolytesHCl, HBr, HI, HNO3, HCIO3, HCIO4, and H2SO4
3 strong bases are strong electrolytes<span>OH, KOH, and NaOH</span>
3 0
3 years ago
2.088 g sample of a compound containing only carbon, hydrogen, and oxygen is burned in an excess of dioxygen, producing 4.746 g
uysha [10]

Answer:

The empirical formula is C3H6O

Explanation:

Step 1: Data given

Mass of the sample =2.088 grams

The mass contains carbon, hydrogen, and oxygen

Mass of CO2 produced = 4.746 grams

Mass of H2O produced = 1.943 grams

Molar mass of CO2 = 44.01 g/mol

Molar mass of H2O = 18.02 g/mol

Atomic mass of C = 12.01 g/mol

Atomic mass of H = 1.01 g/mol

Atomic mass of O = 16.0 g/mol

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass CO2

Moles CO2 = 4.746 grams/ 44.01 g/mol

Moles CO2 = 0.1078 moles

Step 3: Calculate moles C

For 1 mol CO2 we have 1 mol C

For 0.1078 moles CO2 we'll have 0.1078 moles C

Step 4: Calculate mass C

Mass C: moles C * atomic mass C

Mass C: 0.1078 moles * 12.01 g/mol

Mass C= 1.295 grams

Step 5: Calculate moles H2O

Moles H2O = 1.943 grams / 18.02 g/mol

Moles H2O = 0.1078 moles

Step 6: Calculate moles H

For 1 mol H2O we'll have 2 moles H

For 0.1023 moles H2O we'll have 2*0.1078 = 0.2156 moles H

Step 7: Calculate mass H

Mass H = 0.2046 moles * 1.01 g/mol

Mass H = 0.218 grams

Step 8: Calculate mass O

Mass O = 2.088 grams - 1.295 grams - 0.218 grams

Mass O = 0.575 grams

Step 9: Calculate moles O

Moles O = 0.575 grams / 16.0 g/mol

Moles O = 0.0359 moles

Step 10: Calculate the mol ratio

We divide by the smallest amount of moles

C: 0.1078 moles / 0.0359 moles = 3

H: 0.2156 moles / 0.0359 moles = 6

O: 0.0359 moles / 0.0359 moles =1

The empirical formula is C3H6O

8 0
3 years ago
A 1.10 mol sample of krypton gas is collected at a pressure of 427 mmHg and a temperature of 6.0°C. The volume of the sample is
Aleksandr [31]

Answer:

Volume = 44.96L

Explanation:

p = 427mmHg = 0.56atm

R = 0.08206

T 6°C = 279k

V = ?

n = 1.10 mol

using ideal gas equation

pv=nRT

0.56 x V = 1.10 x 0.08206 x 279

0.56 x V = 25.18

V = 25.18/0.56

V = 44.96L

6 0
3 years ago
Nail polish remover containing acetone was spilled in a room 7.2 m × 5.8 m × 3.9 m. Measurements indicated that 6,400 mg of acet
sergeinik [125]

Volume of room  = 7.2 m \times 5.8 m \times  3.9 m

= 162.864 m^{3}

Now, according to conversion factor, convert 6,400 mg to micrograms

Since, 1 mg is equal to 1000 microgram.

Therefore, 6,400 mg  = 6,400 \times 1000

= 6,400,000 micrograms of acetone.

To calculate concentration of acetone, divide volume and evaporated amount of acetone in micrograms.

Thus,

Concentration of acetone  = \frac{6,400,000 microgram}{162.864 m^{3}}

= 39296.5910 microgram per cubic meter or 3.92\times 10^{4} \mu g/m^{3}\simeq 4.0\times 10^{4} \mu g/m^{3}

Hence, concentration of acetone is equal to 4.0\times 10^{4} \mu g/m^{3}

7 0
3 years ago
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