Explanation:
The reaction is as follows.
Standard values of bond energies are as follows.
C-C = 347 kJ/mol
C-H = 414 kJ/mol
C-O = 360 kJ/mol
O-H = 464 kJ/mol
O=O = 498 kJ/mol
C=O = 799 kJ/mol
Hence, calculate the change in enthalpy of the reaction as follows.
= [5(C-H) + 1(C-C) + 1(C-O) + 1(O-H) + 3(O=O)] - [4(C=O) + 6(O-H)]
=
= (4735 - 5980) kJ
= -1245 kJ
Thus, we can conclude that the enthalpy of given reaction is -1245 kJ.
<u>Answer:</u> The molar mass of the gas is 35.87 g/mol.
<u>Explanation:</u>
To calculate the mass of gas, we use the equation given by ideal gas:
PV = nRT
or,
where,
P = Pressure of gas = 945 mmHg
V = Volume of the gas = 0.35 L
m = Mass of gas = 0.527 g
M = Molar mass of gas = ? g/mo
R = Gas constant =
T = Temperature of gas =
Putting values in above equation, we get:
Hence, the molar mass of the gas is 35.87 g/mol.
A. the wax is a both; 1. physical change-solid to liquid.
2. chemical change- burned to CO2 + H20 + heat + carbon as seen as black on the rod
b. the wick is neither; the wick does not change, just provides conduit for wax to flame
c. the glass rod is physical change; the carbon is only deported
HOPE THIS HELPS, IVE ALSO LEARNING BEEN LEARNING THIS RECENTLY