A mass of 35.0 g of an unknown solid initially at 170.0 ∘C is added to an ideal constant-pressure calorimeter containing 100.0 g of water (Cs, water=4.184 J/(g⋅∘C)) initially at 20.0 ∘C. After the mixture reaches thermal equilibrium, the final temperature is recorded to be 38.73 ∘C. What is the specific heat capacity of the unknown solid?

1.70 is the specific heat capacity of the unknown solid.

Explanation:

Data given:

mass of solid = 35 grams

initial temperature = 170 degrees

mass of water = 100 grams

initial temperature = 20 degrees

Final temperature of mixture = 38.73 degrees

specific heat capacity of water = 4.184 J/g°C

specific heat capacity of metal =?

The specific heat capacity will be calculated using the formula:

q = mcΔT

-q solid = q water

-m c (T2-Ti)= m c (T2-Ti)

-35 x c x(38.73-170) = 100 x 4.18 x (38.73 -20)

- 35 x c x(-131.27) = 100 x 4.18 x 18.73

4594 c= 7829.14

c =

c solid= 1.70

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.

c

explanation: