A piece of copper (12.0 g) is heated to 100.0 °C. A piece of chromium (also 12.0 g) is chilled in an ice bath to 0 °C. The specific heat capacity of water is 4.184 J/g ⋅°C.
Both pieces of metal are placed in a beaker containing 200.0 g at 20.0 °C.
(a) Will the temperature of the water be greater than or less than 20.0 °C when thermal equilibrium is reached?
(b) Both pieces of metal are placed in a beaker containing 200.0 g at 20.0 °C. Calculate the final temperature.

(a) Slightly greater than 20.0 °C

(b)

Explanation:

Hello,

In this case, since we are talking about the equilibrium temperature that will be reached when the copper, chromium and water samples get in contact, the following equation is useful to describe such situation:

Thus, in terms of masses, heat capacities and temperatures we consider the final temperature as the unknown:

In such a way, by knowing that the heat capacities of copper and chromium are 0.386 and 0.45 J/(g°C) respectively, by solving for the equilibrium temperature one has:

Hence, the resulting temperature of water turns out slightly greater than 20.0 °C.

Best regards.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

3 1/4 %

explanation: