All categories

3 years ago

ILL BRAINLIST!!

Chemistry

1 answer:

FrozenT [24]3 years ago

8 0

Answer:

In 1859, European rabbits (Oryctolagus cuniculus) were introduced into the Australian wild so that they could be hunted. ... These rabbits are extremely adaptive, which has played a role in their spread across the Australian continent. All the rabbits need is soil that is fit to burrow and short grasses to graze on.

You might be interested in

What are the most enzymes in the body?

Alex787 [66]

Examples of specific enzymes
Lipases – a group of enzymes that help digest fats in the gut.
Amylase – helps change starches into sugars. ...
Maltase – also found in saliva; breaks the sugar maltose into glucose. ...
Trypsin – found in the small intestine, breaks proteins down into amino acids.

4 0

4 years ago

Calculate the number of moles in 2.4g of carbon

Anna71 [15]

Answer:

0.2

Explanation:

1. First, figure out the molar mass of said element(s).

The molar mass of carbon is 12.0107. Whether you round this or leave it as is depends on your's and/or your teacher's personal preference.

2. Next, convert grams to moles by dividing the initial mass of carbon by the molar mass. Round if neccecary.

2.4g ÷ 12.0107g/mol = 0.2mol

6 0

4 years ago

Use the table on the right to calculate each required quantity

ValentinkaMS [17]

(1) The quantity of heat required to melt 175 g Cu is 35.88 kJ.

(2) The substance that releases 21.2 kJ of energy when 1.42 mol of it freezes is iron.

<h3>What is heat of fusion?</h3>

Heat of fusion is the energy required to melt 1 mole of a substance.

<h3>What is heat of vaporization?</h3>

The heat energy required to vaporize 1 mole of a substance has been heat of vaporization.

Heat of fusion of copper (Cu) is given as 13 kJ/mol

Number of moles of 175 g of copper = 175/63.5 = 2.76 moles

Q = nΔH

Q = 2.76 mol x 13 kJ/mol = 35.88 kJ

Thus, the quantity of heat required to melt 175 g Cu is 35.88 kJ.

<h3>Heat of fusion of the substance</h3>

ΔH(fus) = Q/n

where;

n is number of moles
Q is quantity of heat released

ΔH(fus) = 21.2 kJ / 1.42 mol

ΔH(fus) = 14.93 kJ/mol

From the table the substance with latent heat of fusion of 14.9 kJ/mol is iron.

Thus, the substance that releases 21.2 kJ of energy when 1.42 mol of it freezes is iron.

Learn more heat of fusion here: brainly.com/question/87248

#SPJ1

3 0

2 years ago

UCI Chemistry researchers, Prof. F. Sherwood Rowland and Dr. Mario Molina werefirst to discovered in 1973 that chlorofluorocarbo

Olin [163]

Answer:

15.27895 x 10⁶kg of chlorine radical is added to the atmosphere in a year due to 100 million MVACs

Explanation:

Chlorofluorocarbons (CF₂Cl₂) from refrigerants produce chlorine radicals according to the following equation

CF₂Cl₂ → CF2Cl + Cl ⁻ .........(1)

From equation 1, one mole of CF₂Cl₂ produces one mole of Chlorine radical

From the question,

The emission rate of CF₂Cl₂ is 59.5mg/hour/MVAC

In one day the emission rate would be 59.5 x 24hours

= 1428mg/day

In one year, the emission rate would be 1428mg/day x 365days

= 521220mg/year

= 521.220g/year/MVAC

Therefore the emission rate for 100 million MVAC using CF₂CL₂ in a year is

= 52122 x 10⁶g/year/MVAC

= 52122 x 10³kg/year/MVAC

The molar mass of CF₂CL₂ = 120.913g/mol

No of moles of CF₂CL₂ = mass/ molar mass

= 52122 x 10⁶g / 120.913g/mol

= 431 x 10⁶ moles of CF₂Cl₂

From equation 1, since one mole of CF₂Cl₂ produces one mole of Chlorine radical, it implies that

431 x 10⁶ moles of CF₂Cl₂ would produce 431 x 10⁶ moles of chlorine radical,

Therefore, to find the mass of chlorine radical produced, we use the formula

No of moles of chlorine radical = mass/ molar mass

431 x10⁶ moles = mass of chlorine radical /molar mass of chlorine radical

431 x 10⁶ moles = mass/ 35.45g/mol

mass of chlorine = 431 x 10⁶ moles x 35.45 g/mol

= 15278.95 x 10⁶ g

In Kg, the mass = 15,278.95 x 10³kg of cholrine radical

= 15.27895 x 10⁶ Kg of chlorine radical

6 0

3 years ago

1. Based on the observed performance of the air bag models and the amounts of sodium bicarbonate and acetic acid (vinegar) neede

Ira Lisetskai [31]

Sodium bicarbonate and acetic acid are not good substitute for sodium azide in airbags since the require more mass and produce less gas.

<h3>Which is the better chemical for an airbag?</h3>

The chemical equation for the production of nitrogen gas from sodium azide is given below:

NaN₃ → 2 Na + 3 N₂

1 mole or 66 go of sodium azide produces 3 moles or 67.2 L of nitrogen gas.

The equation for the production of carbon dioxide from sodium bicarbonate and acetic acid is given below:

Na₂CO₃ + CH₃COOH → CH₃COONa + CO₂ + H₂O

1 mole, 106 g of Na₂CO₃ and 1 mole, 82 g of CH₃COOH are required to produce 1 mole or 22.4 L of CO₂.

The mass of sodium azide required is less than that of sodium bicarbonate and acetic acid required. Also, sodium azide produces a greater volume of gas. Therefore, sodium bicarbonate and acetic acid are not good substitute for sodium azide in airbags.

In conclusion, sodium azide is a better choice in airbags.

Learn more about airbags at: brainly.com/question/14954949

#SPJ1

7 0

2 years ago