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Ulleksa [173]
3 years ago
12

Ignore the answer I have selected but please help!! Ty in advance, also please explain

Chemistry
1 answer:
weeeeeb [17]3 years ago
4 0

Answer:

Iodine is most reactive because it is very close to having a "full shell" which is 8 electrons so they are "eager" to gain the last electron to became balanced, so that makes it the most reactive. Hope that helps:)

Explanation:

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What is an example of taking action or doing service in the cement industry
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mining of clay limestone and then heated to a certain temperature of 1450⁰ in a cement kiln

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A functional group introduces heteroatoms into a carbon chain to increase
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3 years ago
Enter your answer in the provided box. Calculate the number of moles of CrCl, that could be produced from 49.4 g Cr202 according
Mrrafil [7]

Answer:

0.4694 moles of CrCl₃

Explanation:

The balanced equation is:

Cr₂O₃(s) + 3CCl₄(l) → 2CrCl₃(s) + 3COCl₂(aq)

The stoichiometry of the equation is how much moles of the substances must react to form the products, and it's represented by the coefficients of the balanced equation. So, 1 mol of Cr₂O₃ must react with 3 moles of CCl₄ to form 2 moles of CrCl₃ and 3 moles of COCl₂.

The stoichiometry calculus must be on a moles basis. The compounds of interest are Cr₂O₃ and CrCl₃. The molar masses of the elements are:

MCr = 52 g/mol

MCl = 35.5 g/mol

MO = 16 g/mol

So, the molar mass of the Cr₂O₃ is = 2x52 + 3x35.5 = 210.5 g/mol.

The number of moles is the mass divided by the molar mass, so:

n = 49.4/210.5 = 0.2347 mol of Cr₂O₃.

For the stoichiometry:

1 mol of Cr₂O₃ ------------------- 2 moles of CrCl₃

0.2347 mol of Cr₂O₃----------- x

By a simple direct three rule:

x = 0.4694 moles of CrCl₃

6 0
3 years ago
an engineer wishes to design a container that will hold 12.0 mol of ethane at a pressure no greater than 5.00x10*2 kPa and a tem
OleMash [197]

Answer:

The minimum volume of the container is 0.0649 cubic meters, which is the same as 64.9 liters.

Explanation:

Assume that ethane behaves as an ideal gas under these conditions.

By the ideal gas law,

P\cdot V = n\cdot R\cdot T,

\displaystyle V = \frac{n\cdot R\cdot T}{P}.

where

  • P is the pressure of the gas,
  • V is the volume of the gas,
  • n is the number of moles of particles in this gas,
  • R is the ideal gas constant, and
  • T is the absolute temperature of the gas (in degrees Kelvins.)

The numerical value of R will be 8.314 if P, V, and T are in SI units. Convert these values to SI units:

  • P =\rm 5.00\times 10^{2}\;kPa = 5.00\times 10^{2}\times 10^{3}\; Pa = 5.00\times 10^{5}\; Pa;
  • V shall be in cubic meters, \rm m^{3};
  • T = \rm 52.0 \textdegree C = (52.0 + 273.15)\; K = 325.15\; K.

Apply the ideal gas law:

\displaystyle \begin{aligned}V &= \frac{n\cdot R\cdot T}{P}\\ &= \frac{12.0\times 8.314\times 325.15}{5.00\times 10^{5}}\\ &= \rm 0.0649\; m^{3} \\ &= \rm (0.0649\times 10^{3})\; L \\ &=\rm 64.9\; L\end{aligned}.

4 0
3 years ago
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