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The combustion of an unknown amount of propylene (x moles of C3H6) with air in a prototype space heater produced the following dry exhaust gas molar analysis: 4.27% CO2, 15.05% O2, and 80.68% N2. Determine
a. The actual molar and mass air/fuel ratios.
b. The percent of theoretical air used.
c. The molar percentage of each combustion product before the exhaust gas was dried for this analysis.
the elemental mass percent composition of ascorbic acid (vitamin C) is 40.92% C, 4.58% H, and 54.50% O. Determine the empirical formula
It takes 46.0 to raise the temperature of an 11.2 piece of unknown metal from 13.0 to 25.0. What is the specific heat for the metal?
which observed color band corresponds to the largest energy difference between levels and which is the smallest?
A solution of acid was found to have a hydrogen ion concentration of 0.03 mol dm-3 what is the pH of the solution?
At 700 K, the equilibrium constant for the reaction CO(g) + H2O(g) ? CO2(g) + H2(g) is 5.10. What is G for the reaction at the specific temperature
Identify the oxidizing agent and reducing agent
Arrange the subsequent substances according to their expected lattice energies, listing them from highest lattice energy to the lowest- MgS, KI, GaN, LiBr
The molar heat capacity of a diatomic molecule is 29.1 J/K·mol. Assuming the atmosphere contains only nitrogen gas and there is no heat loss, calculate the total heat intake if the atmosphere warms up by 5°C during the next 50 years in J/mol
Describe the incident and identify the polymeric or explosive materials and discuss the chemical interactions of the material(s) involved in this incident or hazardous properties relevant to the incident.
Calculate %wt of C, H, and O in the compound and find the empirical formula of this compound - What is the weight percent of Cl
Problem- Urea ((NH2)2CO) can be formed from ammonia and carbon dioxide as shown in the following reaction. The ?H° value for this synthesis is -134.0 kJ. Calculate the ?H°f for urea.
Barbituric acid (ka = 1.1x10^-4) is used in the manufacture of some sedatives. For a 0.6733 M solution of barbituric acid, calculate
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