110 g of water (specific heat = 4.184 j/g c) and 100 g of a metal sample (specific heat = 0.397 j/g c) are heated from 25 degrees c to 75 degrees c. which substance required more thermal energy?

Water.

Explanation:

Q = m.C.ΔT, where,

Q is the thermal energy,

m is the mass of the substance ,

C is the specific heat of the substance ,

ΔT is the increase in temperature.

For water,

Q for water = m.C.ΔT = (110 g) (4.184 J/g.°C) (75 °C - 25 °C) = 23012 J.

For the substance,

Q for the substance = m.C.ΔT = (100 g) (0.397 J/g.°C) (75 °C - 25 °C) = 1985 J.

So, it is clear that water (23012 J) requires more thermal energy than the substance (1985 J).

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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: