List 3 ways that scientists investigate and learn about the natural world?

Answer:

The structure for 2 brormocyclopentan amine is given in attached file.

Explanation:

2-bromocyclopentamine (Figure attached) is a synthetic compound which is synthesized by substitution reaction of cyclopentamine and hydrobromide. Its molecular formula and molecular mass are C5H10NBr and 164.05 g/mol respectively.  It is a very reactive compound so it doesn’t available in pure form, it is present in market as a mixture of 2-bromocyclopentamine and Hydrobromide.

Properties:

Its boiling point is 115 °C.

Its melting point is  -75 °C.

It is highly flammable.

It is highly toxic.

It is irritant.

It is corrosive in nature.

Answer: 14.7 L of oxygen gas at 25 degrees celsius and 1.04 atm is needed for the complete combustion of 5.53g of propane

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at NTP, weighs equal to the molecular mass and contains avogadro's number of particles.

According to stoichiometry :

1 mole of propane requires 5 moles of oxygen  

Thus 0.125 moles of propane require= moles of oxygen  

According to the ideal gas equation:'

P = Pressure of the gas = 1.04 atm

V= Volume of the gas = ?

T= Temperature of the gas = 25°C = 298 K  

R= Gas constant = 0.0821 atmL/K mol

n= moles of gas= 0.625

Final answer:

To find the volume of oxygen gas needed for the complete combustion of propane at given conditions, use stoichiometric calculations based on the balanced chemical equation and apply the ideal gas law.

Explanation:

The question is asking for the volume of oxygen gas required for the complete combustion of a given amount of propane at a specified temperature and pressure. To solve this, stoichiometry must be used along with the ideal gas law. The balanced chemical equation for the combustion of propane (C3H8) is:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l)

This equation indicates that one mole of propane reacts with five moles of oxygen. First, calculate the moles of propane by dividing the given mass of propane by its molar mass. Then, use the stoichiometric relationship from the balanced equation to find the moles of oxygen needed. Finally, apply the ideal gas law (PV=nRT) to calculate the required volume of oxygen at the given conditions (remembering to convert temperature to Kelvin and pressure to atm if necessary).

Learn more about Stoichiometry here:

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Answer

its B

Explanation:

B.

Nuclear energy produces little air pollution.

Answer:

When the pressure changes from 1417 psi to  160.186 psi the volume changes from 0.145 L to 0.878 l and the temperature changes from 287 k to 196 k

Explanation:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

Given data:

Initial volume = 0.145 L

Initial pressure = 1417 psi (1417/14.696 =96.42 atm)

Initial temperature = 287 K

Final temperature = 196 K

Final volume = 0.878 L

Final pressure = ?

Formula:

P₁V₁/T₁ = P₂V₂/T₂

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂  = Final temperature

Solution:

P₂ = P₁V₁ T₂/ T₁ V₂  

P₂ = 96.42 atm × 0.145 L × 196 K / 287 K × 0.878 L

P₂  =  2740.26 atm .L.  K  / 251.99 k. L

P₂  = 10.9 atm

atm to psi:

10.9 × 14.696 = 160.186 psi

Answer:

160.186 psi

Explanation:

Electric current passes through a filament of an incandescent bulb, thereby increasing it temperature. When current flows, it contains electrons through the filament to produce light. Typically, incandescent light bulb consists of a glass enclosure that contains tungsten filament. The glass enclosure contains either a vacuum or an inert gas that serves as the filament protection from evaporating. Incandescent light bulbs contain a stem attached at to its base to allow the electrical contacts to run through the envelope without gas or air leaks. 

Answer:

A car battery turning a car on.