What is the mass of a sample that absorbs 32J of energy when it is heated from 274K to 314K and has a specific heat of 0.20 J/gK. *

The answer to your question is 4 g

Explanation:

Data

mass = m = ?

Energy = E = 32 J

Temperature 1 = T1 = 274°K

Temperature 2 = T2 = 314°K

Specific heat = C = 0.20 j/g°K

Formula

     E = mC(T2 - T1)

-Solve for m

     m = E / C(T2 - T1)

-Substitution

      m = 32 / 0.2(314 - 274)

-Simplification

     m = 32 / 0.2(40)

     m = 32 / 8

-Result

     m = 4 g

-Conclusion

   The sample has a mass of 4 g.

Mass of sample is 4 grams

Explanation:

specific heat = s= 0.20 J / gk

ΔT =T₂ - T₁

Where T₁ = 274 k

            T₂ = 314 k

  ΔT = 314 - 274

        =  40 K

Energy absorbed (q) = 32 J

q = msΔT

Make m the subject of formula

m = q / sΔT

   = 32 / 0.2 x 40

   = 32 / 8

   = 4 grams

Therefore, the mass of sample = 4 grams

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: