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What are the sources of error that could happen in the experiment of ''dumas method for determining the molecular weight of volatile liquids''
How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?
Show that the balanced equation obeys the law of conservation of mass.
How many grams of KHP are needed to neutralize 54.63 mL of a 0.1051 M NaOH solution?
A piece of sodium metal reacts completely with water as follows. 2 Na(s) + 2 H2O(l) 2 NaOH(aq) + H2(g) The hydrogen gas generated is collected over water
Tablets from a bottle of commercial aspirin gave a negative test with FeCl3. Several months later, tablets from the same bottle gave a positive test with FeCl3. How do you account for this result? Why?
What is the major disadvantage of using concentrated sulfuric acid (or hydrochloric acid) rather than 85% phosphoric acid for the dehydration of alcohols?
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) In a certain experiment, 4.30 g of NH3 reacts with 7.48 g of O2. Which is the limiting reactant?
a toxicologist studying mustard gas, S(CH2CH2Cl)2, prepares a mixture of 0.675 M SCl2 and 0.973 M C2H4 and allows it to react at room temperature (20.0 c) at equilibrium S(CH2CH2Cl)2 = .350 M. calculate Kp
One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures.
At a particular temperature, K=2.0x10^-6 mol/L for the following reaction: 2CO2 (g) at equilibrium with 2CO(g) + O2 (g) If 2.1 mol CO2 is initially placed into a 4.2 L vessel, calculate the equilibrium concentrations for all of the species.
Drinking water in the USA cannot exceed 0.5 ppm mercury. What mass of mercury is present in 1.3 L of water at this concentration. What is the molar concentration of mercury
If the half-life of a first-order reaction is 4.609 hours what is the instantaneous rate of the reaction in M/day when the concentration of A equals 0.251 M?
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