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Pretend you started with 3.15 g of Panacetin, and you isolated 822 mg of sucrose. What is the percent composition of sucrose in Panacetin?
Suppose that a 2.00-L metal bottle that contains air at 113K and 2.5 atm pressure is sealed off. If we inject 60.0 mL of liquid helium and allow the entire system to warm to room temperature (25°C), what is the pressure inside the bottle?
As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 75.0 atm, what was the volume of the sample? Assume that the temperature was held constant.
What volume (L) of H2 at 745 torr and 20.oC can be prepared from 4.8 g of water? (Atomic weights: Fe = 55.85, O = 16.00, H = 1.008; 1 atm = 760 torr).
Calculate the altitude at which only 10% of the mass of the atmosphre is above and 90% of the mass of the atmosphere is below.
How many calories are required to raise the temperature of 125.0g of water from 50.0 degrees c to 95.0 degrees c?
Draw a flow chart showing the procedure and the observations to be expected at each step with each of the possible cations.
Molecular bromine is 24 per cent dissociated at 1600 K and 1.00 bar in the equilibrium Br2(g) to 2Br(g). Calculate K at (a) 1600K, (b) 2000 K, given that standard enthalpy change = +112 kJ mol-1 over the temperature range.
Write a balanced molecular equation and a net ionic equation for the reaction aluminum hydroxide with a solution of hydrobromic acid. Include the states of each species. a) balanced molecular equation b) net ionic equation
A and B mix to form an ideal solution.what is the Gibbs energy of A in the solution as compare to the Gibbs energy
A reaction mixture initially contains 0.86 M NO and 0.86 M S03. Determine the equiibrium pressure of NO2 if Kc for the reaction at this temperature is 0.0118.
Classify each of the following as an element, compound, homogeneous mixture, or heterogeneous mixture.
At 700.°C, the total pressure of the system is found to be 3.45 atm. If the equilibrium constant KP is 1.52, calculate the equilibrium partial pressures of CO2 and CO.
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