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A 10.0-g sample of a mixture of CH4 and C2H4 reacts with oxygen at 25 degrees celcius at 1 atm to produce CO2 and H20. If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture?
what is the net ionic equation for lead ii nitrate magnesium
A reactant R is being consumed in a first-order reaction. What fraction of the initial R is consumed in 4.0 half-lives
The hydrocarbon benzene C_6_H_6_ boils at 80.1 C. How much energy is required to heat a 1.00 kg of this liquid from 20 C to the boiling point and then changes the liquid completely to a vapor at that temperature
A second-order reaction of the type A+2Bâ†'P was carried out in a solution that was initially 0.050 mol dmâˆ'3 in A and 0.030 mol dmâˆ'3 in B. After 1.0 h the concentration of A had fallen to 0.010 mol dmâ
A quantity of gas under a pressure of 1.78 atm has a volume of 550 cm square. the pressure is increased 2.50atm while the pressure remains constant what is the new volume.
Air at 25°C and 100 kPa has a dew point of 16°C. If you want to remove 50% of the initial moisture in the air (at a constant pressure of 100 kPa), to what temperature should you cool the air
Diethylamine, (C2H5)2NH, is a weak base (pKb=3.16 at 25oC). What is the pH of 0.155 mol/L (C2H5)2NH(aq) at 25oC
All of the following are physical properties of a substance in a liquid state EXCEPT a.indefinite volume b.definite mass c.not easily compressed d.indefinite shape
Consider the compounds with the generic formulas listed below and their corresponding molar solubilities in pure water.
a solution contains 29 g of sucrose c12h22o11 a nonelectrolyte dissolved in 929 g of water. what is the boiling-point
If a pipette was incorrectly calibrated so that it transfers 5% too much solution, would the density you calculated for the liquid tend to be larger or smaller then the correct value. explain.
Calculate a final molarity (M) for a solution if 10. mL of Part "d" is diluted to 0.20 L with pure water. 11 g. Discuss the miscibility of ethylene glycol in water using London dispersion, dipole-dipole, hydrogen bond interactions
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