Butane (C4H10(9), AH = -125.6 kJ/mo) reacts with oxygen to produce carbon dioxide (CO2. AH+ = -393.5 kJ/mol) and water (H20, AH+ = -241.82 kJ/mol) according to the equation below.
2C4H10(g) + 1302(g) → 8C02(g) + 10H2O(g)
What is the enthalpy of combustion (per mole) of C4H10(9)?
Use AH yen-(AHproducts) - ( He reactants)
-2,657.5 kJ/mol
0-5315.0 kJ/mol
--509.7 kJ/mol
O-254.8 kJ/mol

ΔH = -5315kJ/mol

Explanation:

Based on Hess's law, ΔH of a reaction is defined as the sum of the ΔH of the products times their reaction coefficient - The sum of the ΔH of the reactants times their reaction coefficient.

For the reaction of the problem, ΔH is:

ΔH = 8ΔH CO2 + 10ΔH H2O - (2ΔH C4H10 - 13ΔH O2)

Where:

ΔH CO2 = -393.5kJ/mol

ΔH H2O = -241.82kJ/mol

ΔH C4H10 = -125.6kJ/mol

ΔH O2 = 0kJ/mol because O2(g) is the state of oxygen under STP.

Replacing:

ΔH = 8*(-393.5kJ/mol) + 10*(-241.82kJ/mol ) - (2*-125.6kJ/mol  - 13*0kJ/mol)

ΔH = -5315kJ/mol

i believe the answer is c. "baking" is the gerund, while "baking blueberry muffins" would be the gerund phrase. hope this ! : )

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.