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Galina-37 [17]
3 years ago
8

The chart shows the voltage of four electric currents.

Chemistry
2 answers:
masha68 [24]3 years ago
7 0

Answer: The correct option is Current W flows at a higher rate than Current Z.

Explanation: To answer this question, we will require Ohm's law.

Ohm's Law states that the current flowing through a conductor across two points is directly proportional to the voltage difference across that two points.

Mathematically,

V=IR

where, V = voltage

I = Current

R = resistance

For the given question, assuming that the resistance is constant. So, the current is directly proportional to the voltage.

V\propto I

Hence, as the current W is greater of all the given currents so, it will flow at a higher rate.

Therefore, the correct answer is Current W flows at a higher rate than Current Z.

masya89 [10]3 years ago
4 0

Answer:

C

Explanation:

Current X has a lower potential difference than Current Y.

Took test on edge 2020.

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determine mass of water formed when 12.5 L NH3(at298K and 1.50atm) is reacted with 18.9L of O2 (at 323K and 1.1atm)
sasho [114]

The  mass  of water formed  is


<u><em>calculation</em></u>

Use  the  ideal   gas  equation   to  calculate the  moles of  NH3  and O2

that  is  Pv= n RT

where;  P= pressure,  

V=  volume,

n = number  of  moles,

R=gas   constant  = 0.0821  l .atm/ mol.K

make n the formula of  the subject  by diving   both side  by  RT

n =  PV /RT

The   moles of NH3

n= (1.50 atm  x 12.5 L) /(  0.0821 L. atm /mol.k   x 298 K)  =0.766  moles

The  moles  of  O2

=(1.1 atm  x 18.9  L) /  (  0.0821 L. atm/ mol.k   x 323 K) = 0.784  moles


write the reaction  between  NH3  and  O2

4 NH3  + 5 O2  →4 No  +6H2O


from  equation above  0.766  moles of NH3  reacted to produce  

0.766 x 6/4 =1.149 moles of H2O


0.784  moles of O2   reacted to  produce  0.784  x 6/5=0.9408  moles  of H20


since  O2  is totally  consumed, O2  is the limiting  reagent  and therefore  the  moles of H2O  produced=  0.9408  moles


mass  of  H2O  = moles x molar mass

 from  periodic table the  molar mass  of H2O  =  (1 x2)+16= 18  g/mol

mass = 18 g/mol  x 0.9408  moles= 16.93  grams


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Iteru [2.4K]

The enthalpy for the reaction : ΔH = -132

<h3>Further explanation</h3>

Given

Reaction and the enthalpy

Required

the enthalpy

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Hess Law

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A + B = G + C  ΔH = -277

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Add up all the reactions and remove the same compound from two different sides

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