Answer:
<em>The</em><em> </em><em>Typical</em><em> </em><em>Oxidation</em><em> </em><em>number</em><em> </em><em>of</em><em> </em><em>Oxygen</em><em> </em><em>is</em><em> </em><em>–</em><em>2</em><em>.</em>
<em>And</em><em> </em><em>as</em><em> </em><em>the</em><em> </em><em>question</em><em> </em><em>said</em><em>.</em><em>.</em><em>.</em><em> </em><em>its</em><em> </em><em>Oxidation</em><em> </em><em>changes</em><em> </em><em>to</em><em> </em><em>–</em><em>1</em><em> </em><em>when</em><em> </em><em>it</em><em> </em><em>is</em><em> </em><em>in</em><em> </em><em>Peroxides</em><em> </em><em>and</em><em> </em><em>–</em><em>½</em><em> </em><em>w</em><em>h</em><em>e</em><em>n</em><em> </em><em>i</em><em>t</em><em>s</em><em> </em><em>i</em><em>n</em><em> </em><em>SuperOxides</em><em>.</em>
<em>Correct</em><em> </em><em>Answer</em><em> </em><em>:</em><em> </em><em>Option</em><em> </em><em>D</em><em>.</em>
Answer:
B) Δ[C]/Δt = 3,60x10⁻² M⁻¹s⁻¹ [A] [B]
Explanation:
For the reaction A + B → C
The formula for rate of reaction is:
Δ[C]/Δt = k [A] [B]
As you have [A], [B] and Δ[C]/Δt information you can multiply [A] times [B] and take this value as X and Δ[C]/Δt as Y. The slope of this lineal regression will be k.
Thus, you must obtain:
y = 3,60x10⁻² X
Thus, rate of reaction is:
B) Δ[C]/Δt = 3,60x10⁻² M⁻¹s⁻¹ [A] [B]
I hope it helps!
For a first order reaction, the half life is inversely proportional to the rate constant.
The formula is
half life = ln(2)/k = 0.693/k
where k is the rate constant
t = 5.50 minutes
k = ln(2)/5.50 = 0.126 min^-1
Your rate constant is 0.126 min^-1.
Answer:
a)
and 
b)
and 
c)
and 
Explanation:
Temperature of the gas is defined as the degree of hotness or coldness of a body. It is expressed in units like
,
and
These units of temperature are inter convertible.



a) 68°F (a pleasant spring day) to °C and K.
Converting this unit of temperature into
and
by using conversion factor:



b) 164°C (the boiling point of methane, the main component of natural gas) to K and °F
Conversion from degree Celsius to Kelvins and Fahrenheit



c) 0K (absolute zero, theoretically the coldest possible temperature) to °C and °F.




Answer:
1. 0.0637 moles of nitrogen.
2. The partial pressure of oxygen is 0.21 atm.
Explanation:
1. If we assume ideal behaviour, we can use the Law of ideal gases to find the moles of nitrogen, considering that air composition is mainly nitrogen (78%), oxygen (21%) and argon (1%):
2. Now, in order to find he partial pressure of oxygen we need to find the total moles of air, and then the moles of oxygen. Then, we use these results to determine the molar fraction of oxygen, to multiply it with total pressure and get the partial pressure of oxygen as follows:
As you see, the molar fraction and volume fraction are the same because of the assumption of ideal behaviour.