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3 years ago

Write an investigative question

Chemistry

1 answer:

pshichka [43]3 years ago

6 0

Answer:

What happened?

What was the date, time and duration of the incident or behavior?

How many times did this happen?

Where did it happen?

How did it happen?

Did anyone else see it happen? Who? What did they say? What did they do?

Was there physical contact? Describe it. Demonstrate it.

What did you do in response to the incident or behavior?

What did you say in response to the incident or behavior?

How did the subject of the allegation react to your response?

Did you report this to anyone in management? To whom? When? What they say and/or do?

Did you tell anyone about the incident or behavior? Who? What did they say and/or do?

Do you know whether the subject of the allegation has been involved in any other incidents?

Do you know why the incident or behavior occurred?

Do you know anyone else who can shed light on this incident?

Is there anything else you want to tell me that I haven’t asked you?

Explanation:

You might be interested in

These models show the electron structures of two different nonmetal elements.

Soloha48 [4]

Answer: Option (D) is the correct answer.

Explanation:

Valence shell is the shell present on the outermost core of an atom and electrons present in the valence shell are known as valence electrons.

If an atom has completely filled valence shell then it means the atom is not reactive in nature because it is already stable.

But when an atom has less than eight electrons in its valence shell then it means to attain stability the atom will readily attract electrons towards itself.

As the given element 1 has 8 electrons in its valence shell. Hence, it is not reactive in nature but element 2 has 6 valence electrons. So, in order to attain stability element 2 will readily attract 2 electrons from a donor atom.

Thus, we can conclude that element 2 is more reactive because it does not have a full valence shell, so it will attract electrons.

4 0

3 years ago

Gloria’s family built a new deck using building materials made from recycled plastic bottles. As they were heated, the plastics

steposvetlana [31]

Answer:2

Explanation:

6 0

3 years ago

1. Methane (CH4) combusts as shown in the equation below. If 3 moles of methane were used in the combustion, what would be the c

umka2103 [35]

Answer:

The change in enthalpy in the combustion of 3 moles of methane = -2406 kJ

Explanation:

Step 1: The balanced equation

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) ΔH = -802 kJ

Step 2: Given data

We notice that for 1 mole of methane (CH4), we need 2 moles of O2 to produce : 1 mole of CO2 and 2 moles of H20.

The enthalpy change of combustion, given here as Δ H , tells us how much heat is either absorbed or released by the combustion of one mole of a substance.

In this case: we notice that the combustion of 1 mole of methane gives off (because of the negative number), 802.3 kJ of heat.

Step 3: calculate the enthalpy change for 3 moles

The -802 kj is the enthalpy change for 1 mole

The change in enthalpy for 3 moles = 3* -802 kJ = -2406 kJ

The change in enthalpy in the combustion of 3 moles of methane = -2406 kJ

5 0

3 years ago

A gas at STP has a volume of 1.5 L. What will the pressure be if it is at 26° C occupying .75 L

andrey2020 [161]

Answer:

P₂ = 2.19 atm

Explanation:

Given data:

Initial volume = 1.5 L

Initial pressure =1 atm

Initial temperature = 273K

Final temperature = 26°C (26+273 = 299 K)

Final volume = 0.75 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 = 1 atm × 1.5 L × 299 K / 273 K × 0.75 L

P₂ = 448.5 atm .L. K / 204.75 K.L

P₂ = 2.19 atm

6 0

3 years ago

How many grams of N2 can be produced when 6.50 g of O2 reacts?

Olenka [21]

Answer:

3.79 g of N2.

Explanation:

We'll begin by writing the balanced equation for the reaction.

This is given below:

4NH3 + 3O2 → 2N2 + 6H2O

Next, we shall determine the mass of O2 that reacted and the mass of N2 produced from the balanced equation.

This is illustrated below:

Molar mass of O2 = 16x2 = 32 g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96 g

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 from the balanced equation = 2 x 28 = 56 g

Summary:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Finally, we shall determine the mass of N2 produced by reacting 6.50 g of O2.

This can be obtained as follow:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Therefore, 6.50 g of O2 will react to produce = (6.50 x 56)/96 = 3.79 g of N2.

Therefore, 3.79 g of N2 were obtained from the reaction..

4 0

3 years ago