The chemical formula of ammonia is written as NH3 we can just use the ratio of the atoms since we are not given the reaction. We also make use the avogadro's number to convert from moles to molecules. We calculate as follows:
5.01 x 10^-4 g H2 ( 1 mol / 2.02 g H2 ) ( 2 mol NH3 / 3 mol H2 ) ( 6.022x10
^23 molecules / 1 mol ) = 9.96 x 10^19 molecules NH3
Ethanol contains an alcohol group (-OH), which includes hydrogen bonding. Hydrogen bonding is stronger than other IMFs such as Van der Waals forces and Dipole-Dipole.
Ethene only has Van der Waals forces as it is an alkene with only C-H or C-C bonds. These means that the forces are not as strong.
Since ethanol contains hydrogen bonding, it will take a higher temperature in order to break these bonds, and thus results in a higher boiling point than ethene.
<u>Answer:</u> The Gibbs free energy of the reaction is -445 J/mol.
<u>Explanation:</u>
The chemical equation for the conversion follows:
The expression for of above equation is:
We are given:
[Glyceraldehyde-3-phosphate] = 0.00400 M
[Dihydroxyacetone phosphate] = 0.100 M
Putting values in above equation, we get:
Relation between standard Gibbs free energy and equilibrium constant follows:
where,
= Standard Gibbs free energy = 7.53 kJ/mol = 7530 J/mol (Conversion factor: 1kJ = 1000J)
R = Gas constant =
T = temperature = 298 K
Putting values in above equation, we get:
Hence, the Gibbs free energy of the reaction is -445 J/mol.
Answer:
0.0063 mol
Explanation:
Step 1: Write the balanced combustion equation
C₈H₁₈(l) + 12.5 O₂(g) ⇒ 8 CO₂(g) + 9 H₂O(g)
Step 2: Establish the appropriate molar ratio
According to the balanced equation, the molar ratio of C₈H₁₈ to CO₂ is 1:8.
Step 3: Calculate the number of moles of C₈H₁₈ needed to produce 0.050 moles of CO₂
0.050 mol CO₂ × 1 mol C₈H₁₈/8 mol CO₂ = 0.0063 mol C₈H₁₈