Manganese reacts with hydrochloric acid to produce manganese(ii) chloride and hydrogen gas. mn(s)+2hcl(aq) ? mncl2(aq)+h2(g)
part a when 0.650g mn is combined with enough hydrochloric acid to make 100.0 ml of solution in a coffee-cup calorimeter, all of the mn reacts, raising the temperature of the solution from 23.0? c to 28.2? c. find ? hrxn for the reaction as written. (assume that the specific heat capacity of the solution is 4.18 j/g? c and the density is 1.00 g/ml.) express your answer using three significant figures. ? hrxn = kj

The enthalpy change of the reaction for given amount of manganese is 181.2 kJ

Explanation:

To calculate mass of solution, we use the equation:

Density of solution = 1.00 g/mL

Volume of solution = 100.0 mL

Putting values in above equation, we get:

where,

q = heat absorbed

m = mass of solution = 100 g

c = specific heat capacity of solution = 4.18 J/g.°C

= change in temperature =

Putting values in above equation, we get:

Given mass of manganese = 0.650 g

Molar mass of manganese = 55 g/mol

Putting values in above equation, we get:

where,

= amount of heat absorbed = 2173.6 J = 2.174 kJ   (Conversion used:  1 kJ = 1000 J)

n = number of moles = 0.012 moles

= enthalpy change of the reaction

Putting values in above equation, we get:

Hence, the enthalpy change of the reaction for given amount of manganese is 181.2 kJ

the answer would be b i believe