A piece of metal of mass 27 g at 93° C is placed
in a calorimeter containing 59.2 g of water at
21°C. The final temperature of the mixture is 34.9 ° C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings.
Answer in units of J/g. ° C

1.586 J/g°C

Explanation:

So, we have the formula .

Since heat released by the metal is = to the heat absorbed by the water (because they eventually become the same temperature in solution), we can say

Plugging in, we get:

Solving, we get J/g°C.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :