Consider the reaction H2CO(g) + O2(g)CO2(g) + H2O(l) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.63 moles of H2CO(g) react at standard conditions. S°surroundings = J/K

3,116J/K

Explanation:

This question asks to calculate the entropy change of the surroundings.

To do this, we need the standard enthalpy of formation ΔfH° of the reacting species and products first:

We should observe that standard enthalpy if formation of O2 is zero. We proceed with the rest of the species.

H2CO = -109.5KJ/mol

CO2 = -393.5KJ/mol

H2O = -285.8KJ/mol

Now, we calculate the standard change of enthalpy of the reaction as:

ΔHrxn = ΔHproduct - ΔHreactant = (-285.8 - 393.5) +(109.5) = -569.8 KJ/mol

The relationship between the entropy and the standard formation enthalpy is given as

The relationship is:

ΔSosurroundings = - ( ΔHof/ T)

We convert the standard enthalpy of formation to joules first = -569.8 * 10^3 Joules

Using the formula above at a temperature of 298k, the entropy change would be:

-(-569.8 * 10^3)/298 = 1912J/K

Now, we know that 1.63 moles of H2CO reacted. We also need to know the coefficient of the H2CO in the reaction which is 1.

We thus have:

1.63 mol H2CO(g) * (1912J/K * 1 mol H2CO) = 3116J/K

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:

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