Given the following reactions, what is the overall enthalpy change for the following reaction? NH3(g) + HCl(g)  NH4Cl(s) Reaction H° (kJ) N2(g) + 3 H2(g)  2 NH3(g) –92 H2(g) + Cl2(g)  2 HCl(g) –185 N2(g) + 4 H2(g) + Cl2(g)  2 NH4Cl(s) –629

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

it's c (engineer's do their work with mechanical stuff not on any living being)