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erica [24]
3 years ago
10

What is the limiting reactant when 5.6 moles of aluminum react with 6.2 moles of water?

Chemistry
2 answers:
alexira [117]3 years ago
7 0

The limiting  reactant  when 5.6  moles   of aluminium react  with  6.2  moles   of water   is

      water( H2O)


      <u><em>Explanation</em></u>

The  balanced    equation is as below

2 Al +3 H2O  →  Al2O3  +3 H2

The mole ratio  of Al :Al2O3  is 2:1  therefore  the  moles  of  Al2O3

  = 5.6 x1/2  =  2.8  moles


The   mole  ratio  of H2O: Al2O3  is 3:1 therefore  the  moles  of Al2O3  produced

                 = 6.2  x1/3= 2.067  moles


since  H2O  yield  less  amount  of Al2O3 ,  H2O   is  the limiting reagent.

nika2105 [10]3 years ago
4 0

<u>Given:</u>

Moles of Al = 5.6 moles

Moles of H2O = 6.2 moles

<u>To determine:</u>

The limiting reagent

<u>Explanation:</u>

The chemical reaction is-

2Al + 3H2O → Al2O3 + 3H2

- Based on stoichiometry; 2 moles of Al forms 1 mole of Al2O3

Therefore, 5.6 moles of Al would give: 5.6 Al * 1 Al2O3/2 Al = 2.8 moles Al2O3

-Similarly; 3 moles of H2O forms 1 mole of Al2O2

Therefore, 6.2 moles of H2O would give: 6.2 H2O * 1 Al2O3/3 H2O = 2.07 moles Al2O3

Ans: Since the amount (moles) of Al2O3 formed from H2O is less, water is the limiting reagent.

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3 years ago
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At what temperature would 2.10moles of N2 gas have a pressure of 1.25atm and fill a 25.0 L tank
hodyreva [135]

Answer:

\large \boxed{\text{-92 $^{\circ}$C}}

Explanation:

We can use the Ideal Gas Law and solve for T.

pV = nRT

Data  

p = 1.25 atm

V = 25.0 L

n = 2.10 mol

R = 0.082 06 L·atm·K⁻¹mol⁻¹

Calculations

1. Temperature in kelvins

\begin{array} {rcl}pV & = & nRT\\\text{1.25 atm} \times \text{25.0 L} & = & \rm\text{2.10 mol} \times 0.08206 \text{ L}\cdot\text{atm}\cdot\text{K}^{-1}\text{mol}^{-1} \times T\\31.25&=&0.09847T\text{ K}^{-1}\\T& = &\dfrac{31.25}{\text{0.098 47 K}^{-1}}\\\\& = &\text{181 K}\end{array}

2. Temperature in degrees Celsius

\begin{array} {rcl}T & = & (181 - 273.15) \, ^{\circ}\text{C}\\& = & -92 \, ^{\circ}\text{C}\\\end{array}\\\text{The temperature of the gas is $\large \boxed{\mathbf{-92 \, ^{\circ}}\textbf{C}}$}

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