What final temperature will be attained by a 250. g sample of Cu at 20.0oC if it absorbs 1000 J of heat? Cu 's c = 0.39 J/(g oC

30.26 °C

Explanation:

From the question,

Q = cm(t₂-t₁) Equation 1

Where Q = Heat, c = specific heat capacity of Cu, m = mass of Cu, t₁ = Initial temperature, t₂ = Final temperature.

Given: Q = 1000 J, c = 0.39 J/g.°C, t₁ = 20°C, m = 250 g

Substitute into equation 1 and solve for t₂

1000 = 250×0.39(t₂-20)

250×0.39(t₂-20) = 1000

97.5(t₂-20) = 1000

(t₂-20) = 1000/97.6

(t₂-20) = 10.26

t₂ = 10.26+20

t₂ = 30.26 °C

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: