Tin metal reacts with hydrogen fluoride to produce tin (II) fluoride and hydrogen gas according to the following balanced equation. Sn(s)+ 2HF(g) → SnF₂(s)+H₂(g) How many moles of hydrogen fluoride, HF, are required to react completely with 75.0g of tin? What information are you given?

g of Sn
mol of Sn
mol of HF
g of HF

Explanation is in the file

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some sources quote the lethal dose, for an average 170lbs opiate-naive individual is between 75 and 375 mg

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol