3. Butane (C4H10) releases 2877 kJ per mole during a standard combustion reaction in air.

a. What is the balanced thermochemical equation for this reaction?

b. How much heat will be released when 200.0 g of butane is burned?

1.  The balanced thermochemical equation for the reaction is;

2C4H10 (g) + 13O2 (g) > 8CO2 (g) + 10H20 (g)

2. Heat when 200g of butane is burned is 9925.65 kJ of heat

Explanation:

2 moles of butane reacts with oxygen in excess to produce carbon iv oxide and water

If 1 mole releases 2877kJ of heat

2 moles will release (2 * 2877kJ) of heat

= 5754 kJ of heat.

The mass of butane used is 200g and converting it to moles we have;

n = mass / molar mass

molar mass of butane = (12 *4 + 1 *10) = 58 g/mol

So therefore n = 200 g/ 58 g/mol

n= 3.45 moles of butane.

If 1 mole of buatne releases 2877 kJ of heat

3.45 moles will release ( 3.45 * 2877 kJ ) of heat

= 9925.65 kJ of heat

9925.65 kJ of heat is released when 200 g of butane is burned.

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: