How many grams of a stock solution that is 87.0 percent h2so4 by mass would be needed to make 200 grams of a 35.5 percent by mass solution? show all of the work needed to solve this problem

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81.609 grams

Explanation:-

In a 35.5% by mass solution of 200 grams

Amount of H2SO4 = 200 x 35.5/100

= 71 grams

Let the amount of stock solution required be G grams

So 87% of G grams should have the same amount of H2SO4 by mass as 71 grams.

∴ G x 87/100 = 71

G = 71 x 100/87

= 81.609 grams

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

i wish i could but this one is weird give me abc and i can solve it.