3.4 moles of solid cuso4 is added to 1.8 l of water and allowed to dissolve. will all the solid dissolve?

                     Yes, all the solid will dissolve.

Explanation:

                    To solve this problem we will first find the solubility of CuSO₄ at given temperature (in this case we will assume the temperature to be 20 °C. According to reported data 37.8 g of CuSO₄ can be dissolved in 100 ml of H2O at 20 °C.

                    While we are provided with moles of CuSO₄ and volume is given in Liters. So, we will convert moles to mass as,

                                   Mass  =  Moles × Molar Mass

                                   Mass  =  3.4 mol × 159.60 g/mol

                                   Mass  =  542.64 g

Secondly, we will convert Liters to milliliters as,

                                  Milliliters  =  Liters × 1000

                                  Milliliters  =  1.8 × 1000

                                  Milliliters  =  1800 ml

Therefore,

According to reference data,

                     37.8 g CuSO₄ dissolves in  =  100 ml of water

So,

            542.64 g CuSO₄ will dissolve in  =  X ml of water

Solving for X,

                      X  =  542.64 g × 100 ml / 37.8 g

                      X =  1435.55 ml of Water

This means that we are provided with greater amount of water (i.e. 1800 m). Hence, the given amount of CuSO₄ will completely dissolve in 1.8 L of water and the solution formed is unsaturated and can dissolve further CuSO₄.

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:

b is the correct answer

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