I need help on these questions 2. A chemistry student added 225 grams of aluminu

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I need help on these questions

2. A chemistry student added 225 grams of aluminum at es.0 c to 115 grams of water at 23.0" Cin a perfect calorimeter. The final temperature of the aluminum-water mixture was 414 C, Use this student's data to calculate the specific heat of aluminum in joulesugram c 3, A cubic block of uranium metal specific heat m 0.1171 g at 200.0 "C is dropped into 100 Ler 4.211, Ig 7 c 1) at 25.5 "C of heavy water (specific heat The final temperature of the uranium and the deuterium oxide mixture is 28,5 c. Glven the densities of uranium N19.05 akmay and deute rum oxide ll g/mL what is the length or the side of the uranium cube? To solve for this you will have to solve a-c first. Determine the mass er uranium dropped into the Do we the heat lost by the uranium equals the heat gained by the water using the equation we dscussed in b use the density equation length using the equation that relates volume and length e Ho was placed in a constant-pressure 4, 175.0 g pul rimeter and chi 100 9,80 g puree Hso to 19,a 10.0 was added, stirred and the temperature rase al What mass increased in temperature? What was At What was the chemical reaction?

Explanation / Answer

There are multiple questions here . i am allowed to answer only 1 at a time. I will answer 1st one for you. Please ask other as different question
2)
specific heat capacity of water = 4.18 J/g oC
use:
Heat lost by aluminium = heat gained by water
mAl* CAl* (TiAl - Tf) = mW * CW*(Tf - Tiw)
225*CAl*(85 - 41.4) = 115*4.18*(41.4 - 23)
225*CAl* 43.6 = 8844.88
CAl = 0.9 J/g oC
Answer: 0.9 J/g oC

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