Molar mass MgS2O3 = <span> 136.43 g/mol
185 g x 1 mole MgS2O3 / 136.43 => 1.356 moles
hope this helps!</span>
The answer is: "second order" .
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Answer:
80.13g of SO2
Explanation:
4FeS2 + 11O2 —> 2Fe2O3 + 8SO2
Molar Mass of FeS2 = 55.8 + (2x32) = 119.8g/mol
Mass of FeS2 from the balanced equation = 4 x 119.8 = 479.2
Molar Mass of SO2 = 32 + (16x2) = 32 + 32 = 64g/mol
Mass of SO2 from the balanced equation = 8 x 64 = 512g
From the equation,
479.2g of FeS2 produced 512g of SO2.
Therefore, 75g of FeS2 will produce = (75 x 512)/479.2 = 80.13g of SO2
1)a) 2.4/4=0.6
b)250x10^(-3)/12=1/48g
c)15/58.5=10/39
d)40/256.8=50/321g
a)1.2x39.1=46.92g
b)75x2=150g
c)0.25x18=4.5
d)0.15x159.6=23.94g
We can use the dilution equation to find the volume of nitric acid needed to prepare a dilute solution
c1v1 = c2v2
c1 is concentration of concentrated solution and v1 is volume of concentrated solution
c2 is concentration of diluted solution and v2 is volume of diluted solution to prepared
substituting the equations
9.00 M x V = 1.25 M x 6.50 L
V = 0.903 L
903 mL of concentrated solution is required