(based on q = -sm∆t)

list the metals in order of increasing specific heat.

the metals are

-brass with a specific heat of 0.418 j/g°c

-aluminum with a specific heat of 0.734 j/g°c

-tin with a specific heat of 0.246 j/g°c

-zinc with a specific heat of 0.419 j/g°c

Sn < Brass ≈ Zn <   Al  

Step-by-step explanation:

                      Sn   < Brass  ≈   Zn   <   Al

C/J·°C⁻¹g⁻¹: .0.246 <  0.418 ≈ 0.419 < 0.734

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

i think so it’s will be b yes i believe its