All categories

4 years ago

To reduce the amount of CO2 that escapes from a bottle of carbonated beverage when you open the cap, you should

Chemistry

1 answer:

notka56 [123]4 years ago

6 0

Answer:

Explanation:

i havnt done this in school yet but my idea is that shaking the bottle makes the co2 float to the top, then when you open it the presure will release and the co2 with rush out

You might be interested in

1. Convert 12,350 fluid Ounces into gallons.

LuckyWell [14K]

Answer: 12350 = 484375 us

Explanation:

6 0

3 years ago

Read 2 more answers

How many moles of hydrogen atoms are there in 1.25 x 1025 molecules of ethane? (C2H6)

krek1111 [17]

Answer:

124.56 moles of Hydrogen atoms.

Explanation:

We'll begin by calculating the number of moles of ethane that contains 1.25×10²⁵ molecules. This can be obtained as follow:

From Avogadro's hypothesis, 1 mole of any substance contains 6.02x10²³ molecules. This implies that 1 mole of ethane also contains 6.02x10²³ molecules.

Thus, 6.02x10²³ molecules are present in 1 mole of ethane.

Therefore, 1.25×10²⁵ molecules are present in = 1.25×10²⁵/6.02x10²³ = 20.76

Therefore, 20.76 moles of ethane contains 1.25×10²⁵ molecules.

Finally, we shall determine the number of mole of Hydrogen in 20.76 moles of ethane. This can be obtained as follow:

Ethane has formula as C2H6.

From the formula, 1 mole of ethane, C2H6 contains 6 moles of Hydrogen atoms.

Therefore, 20.76 moles of ethane will contain = 20.76 × 6 = 124.56 moles of Hydrogen atoms.

Therefore, 1.25×10²⁵ molecules of ethane contains 124.56 moles of Hydrogen atoms.

7 0

4 years ago

A chemical company makes two brands of antifreeze. The first brand is 65% pure antifreeze, and the second brand is 90% pure anti

mojhsa [17]

When two material with different concentrations of the same active ingredient are mixed, the active ingredient before and after mixing remains constant. If the volume of the first brand is assigned x gallons, the volume of the second brand is (160-x) gallons. Therefore, according to the above principle, (65%)(x) + (90%)(160-x) = (70%)(160), 0.65x+ 144-0.9x = 112, x=128 gallon. 128 gallon of the first brand (65%) and 160-128 = 32 gallon of the second brand (90%) of antifreeze must be used.

3 0

4 years ago

How much heat energy, in kilojoules, is required to convert 53.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer

ANTONII [103]

Answer:

25.2 kJ of heat energy is required to convert 53.0 g of ice at −18.0 ∘C to water at 25.0 ∘C

Explanation:

Data: mass of ice = m = 53.0 g

Temperature of ice = T1 = -18.0 ∘C

Temperature of water = T2 = 25.0 ∘C

Change in Temperature = ΔT : T2-T1

Specific heat of ice = c(i) = 2.09 J/g . ∘C

Specific heat of water = c(w) = 4.18 J/g . ∘C

Enthalpy of fusion of water (when convert from ice to water) = ΔH(f) : 334 J/g

Enthalpy of vapourization of water (when convert from water to gas) = ΔH(v) :2250 J/g

Total heat required = q = ?

Solution: Heat required to melt the ice

T1 = -18 ∘C

T2 = 0 ∘C

Q1 = m x c(i) x ΔT

Q1 = 53.0 x 2.09 x (0-(-18))

Q1 = 53.0 x 2.09 x 18

Q1 = 1993.86 J is required by ice to reach to its

melting point.

Heat required to convert the ice into water

Q2 = ΔH(f) x m

Q2 = 334 x 53.0 = 17702 J is required by ice to

convert into water.

Heat required by water to reach at 25 ∘C

T1 = 0 ∘C

T2 = 25 ∘C

Q3 = m x c(w) x ΔT

Q3 = 53.0 x 4.18 x (25-0)

Q3 = 5538.5 J is required by water to reach at

25∘C .

Total heat required by 53.0 g of ice at −18.0 ∘C

to water at

25.0 ∘C

q = Q1 + Q2 + Q3

q = 1993.86 J + 17702 J + 5538.5 J

q = 25234.36 J is the total heat required 53.0 g

of ice at −18.0 ∘C to water at 25.0 ∘C.

Conversion from Joule (J) to Kilojoule (kJ)

1000 J = 1 kJ

q = 25234.36 J/1000

q = 25.23436 kJ

Conversion of heat in kJ to three significant

figures

q = 25.2 kJ

8 0

4 years ago

Anions have more ___ then __

never [62]

C protons, elctrons 093939393

6 0

3 years ago