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A sample of a compound contains 3.6 g of Boron and 1 g of Hydrogen. What is the compound’s empirical formula?
If the half of a reactant in a 1st order reaction is 25 minutes, then what is the extent of reaction after 2 minutes?
A 1.397 g sample of thymol, C 10 H 14 O (s) (a preservative and a mold and mildew preventative),
is burned in a bomb calorimeter assembly. The temperature increase is 11.23°C, and the heat
capacity of the bomb calorimeter is 4.68 kJ/°C. What is the heat of combustion of thymol,
expressed in kJ/mol C 10 H 14 O?
The heat of combustion of 2-propanol at 298.15 K, determined in a bomb calorimeter, is -
33.41 kJ/g. For the complete combustion of one mole of 2-propanol, determine (a) ΔE, and (b)
ΔH.
How many moles of oxygen will take up a volume of 2.5 liters if the pressure is 121.59 kPa and the temperature is 25oC?
1. A hardworking human brain, perhaps one that is grappling with physical chemistry, operates at about 25 J/s. What mass of glucose must be consumed to sustain that metabolic rate for an hour? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide gas and liquid water at 25°C is 2828 kJ. Ans. 5.7g
1. How much energy is available for sustaining muscular and nervous activity from the combustion of 1.00 mol of glucose molecules under standard conditions at 37°C (blood temperature)? The standard entropy of reaction is +182.4J/ K mol and the standard reaction enthalpy is – 2808 kJ/mol. Ans.2865 kJ/mol
Theoretical yield of the silver chromate
How many degrees can iron be changed if 9,000 joules of energy are lost from 5 Kg pieces
A concentration (P) of gaseous hydrogen peroxide (H2O2(g)) was placed into an evacuated container of fixed volume that was kept at 855K. At this temperature some of the gaseous hydrogen peroxide decomposed to form gaseous hydrogen (H2(g)) and gaseous oxygen(O2(g)) until an equilibrium was established. The pressure in the container was measured to be 2.88 x 103 mmHg. The equilibrium constant (Kc) was measured to have a value of 0.176 for the decomposition reaction.
A concentration (Q) of gaseous hydrogen peroxide was then carefully removed from the mixture in the container and the reaction was allowed to reach equilibrium for the second time. At the second equilibrium the concentration of gaseous hydrogen was found to be 32.6% less than it was at the first equilibrium. The values of P and Q, respectively are:
