A52.4 g sample of brass is put into a calorimeter (see sketch at right) that contains 150.0 g of water. the brass sample starts off at 95.1 °c and the temperature of the water starts off at 15.0 °c. when the temperature of the water stops changing it's 17.6°c. the pressure remains constant at 1 atm. container water calculate the specific heat capacity of brass according to this experiment.

The specific heat capacity of brass is 0.402 J/g°C

Explanation:

Step 1: Data given

Mass of the sample of brass = 52.4 grams

Mass of water = 150.0 grams

Initial temperature of brass sample = 95.1 °C

Initial temperature of water = 15.0 °C

Final temperature = 17.6°C

Pressure = 1atm

Specific heat capacity = 4.184 J/g°C

Step 2: Calculate specific heat capacity of brass sample

Heat lost by the brass sample = heat won by water

Q = m*c*ΔT

Qbrass = -Qwater

m(brass)*c(brass)*ΔT(brass) = -m(water) *c(water) * ΔT(water)

⇒mass of brass sample = 52.4 grams

⇒ c(brass) = TO BE DETERMINED

⇒ ΔT = T2 - T1 = 17.6 °C - 95.1 °C = -77.5 °C

⇒ mass of water = 150.0 grams

⇒ c(water ) = 4.184 J/g°C

⇒ ΔT(water) = 17.6 °C - 15 °C = 2.6°C

52.4g * c(brass) * (-77.5°C) = -150.0g * 4.184 J/g°C * 2.6 °C

-4061 * c(brass) = -1631,76

c(brass) = 0.402 J/g°C

The specific heat capacity of brass is 0.402 J/g°C

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

pie chart because it is in percents ( % )