2. a. i. Iron reacts with H2SO4 according to the equation: Fe(s) + H2SO4(aq) - → FeSO4(aq) + H2(g). Calculate the mass of FeSO4 that would be produced by 0.5mole of Fe. ii. Calculate the volume of CO2 produced when 5.8g of Na2CO3 reacted with excess HNO3 Na2CO3(s) + 2HNO3(aq) 2NaNO3(aq) + CO2(g) +H20(l)

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.

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