5.35g of solid ammonium chloride, NH₄Cl(s), was added to water to form 25.0g of solution. The maximum decrease in temperature was 14 K. What is the enthalpy change, in kJmol^-1, for this reaction? (Molar mass of NH₄Cl = 53.5gmol^-1; the specific heat capacity of the solution is 4.18 Jg^-1K^-1)

A. \(\Delta H =  + \frac{{25.0 \times 4.18 \times \left( {14 + 273} \right)}}{{0.1 \times 1000}}\)

B. \(\Delta H =  - \frac{{25.0 \times 4.18 \times 14}}{{0.1 \times 1000}}\)

C. \(\Delta H =  + \frac{{25.0 \times 4.18 \times 14}}{{0.1 \times 1000}}\)

D. \(\Delta H =  + \frac{{25.0 \times 4.18 \times 14}}{{1000}}\)

C