A student carried heated a 25.00 g piece of aluminum to a temperature of 100°C, and placed it in 100.00 g of water, initially at a temperature of 10.0°C. Determine the final temperature of the system (aluminum and water)

cH2OB4.18J/gc

c Aluminum .900 j/g c

The final temperature of the system is 14.60°C

Explanation:

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

The equation used to calculate heat released or absorbed follows:

     ......(1)

where,

q = heat absorbed or released

= mass of aluminium = 25.00 g

= mass of water = 100 g

= final temperature = ?°C

= initial temperature of aluminium = 100°C

= initial temperature of water = 10°C

= specific heat of aluminium = 0.900 J/g°C

= specific heat of water= 4.18 J/g°C

Putting values in equation 1, we get:

Hence, the final temperature of the system is 14.60°C

answer; talc and gypsum;

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.