A sample of brass is put into a calorimeter (see sketch at right) that contains of water. The brass sample starts off at and the temperature of the water starts off at . When the temperature of the water stops changing it's . The pressure remains constant at . Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to significant digits.

Complete Question

The complete question is shown on the first uploaded image

The specific heat is  

Explanation:

From the question we are told that

    The mass of  the sample is  

     The mass of the water is  

     The initial temperature of the sample is  

     The initial temperature of the water is  

     The final temperature of the water is  

Note the final temperature of water is equal to the final temperature of brass sample

    The pressure is  

Generally for according to the law of energy conservation

    The heat lost by sample  =  The heat gain by water

The heat lost by brass sample is  mathematically evaluated as    

Where is the specific neat of the brass sample

The heat gained  by water is  mathematically evaluated as          

where is the specific heat of water which has a constant value of  

So

substituting values

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2