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statuscvo [17]
2 years ago
7

Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide. 5 C (s) + 2 SO2

(g) --> CS2 (l) + 4 CO (g) How many moles of CS2 form when 2.79 mol C react?
Chemistry
1 answer:
lutik1710 [3]2 years ago
5 0
I got 0.558 moles of CS2
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Properties of group 7 (aka. The Halogens)?
ella [17]
Halogens can be characterized as :

1) High Electronegativity 
2) Low melting & boiling points
3) Forms Ionic compounds
4) Non-metallic in nature

Hope this helps!
7 0
3 years ago
How many particles would be found in a 1.224 g sample of K2O
lbvjy [14]

Answer:

9.96*10^21

Explanation:

Molar mass of K2O=29*2+16

= 74g per mol

number of moles in the sample= 1.224/ 74

=0.1654

Number of particles in 1 mole=6.0221409*10^23

Number of particles= 0.01654*6.0221409*10^23

=9.96*10^21

4 0
3 years ago
Read 2 more answers
A 2.0-liter aqueous solution contains a total of 3.0 moles of dissolved NH4Cl at 25°C and standard pressure.
vladimir1956 [14]
The molarity is a concentration unit which defined as the number of moles of solute divided by the number of liters of solution. So the molarity of the solution is 3/2=1.5 mol/L.
7 0
2 years ago
Read 2 more answers
What mass of aluminum is produced by the decomposition of 5.0 kg al2o3?
Nina [5.8K]
The  mass for  of aluminum that is produced  by  the decomposition  of  5.0 Kg Al2O3 is 2647 g or 2.647  Kg

          calculation
  Write  the equation for decomposition  of Al2O3

Al2O3 = 2Al  + 3 O2

find the  moles  of  Al2O3 =  mass/molar mass

convert  5 Kg  to g   = 5 x1000 = 5000 grams
molar mass of  Al2O3 =  27 x2 + 16 x3  = 102 g/mol

 moles =5000 g/  102 g/mol = 49.0196 moles

by use  of mole ratio between Al2O3 to  Al  which is 1:2  the moles of Al = 49.0196 x2 =98.0392  moles


mass of  Al = moles x molar  mass

= 98.0392 moles x  27g/mol = 2647  grams  or 2647/1000 = 2.647 Kg


7 0
3 years ago
Read 2 more answers
The reaction 2a + b --> c + d has an activation energy of 80.0 kj/mol. at 320°c, the rate constant k = 1.80 x 10-2 l mol-1 s-
Naddik [55]
To determine the k for the second condition, we use the Arrhenius equation which relates the rates of reaction at different temperatures. We do as follows:

ln k1/k2 = E / R (1/T2 - 1/T1) where E is the activation energy and R universal gas constant.

ln 1.80x10^-2 / k2 = 80000 / 8.314 ( 1/723.15 - 1/593.15)

k2 = 0.3325 L / mol-s
5 0
3 years ago
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