Search & Filtering
Magnesium oxide and nickel oxide withstand high temperatures. However, they do melt when the temperature is high enough and the behaviour of mixtures of the two is of considerable interest to the ceramics industry. Draw the temperature–composition diagram for the system using the data below, where x is the mole fraction of MgO in the solid and y its mole fraction in the liquid.
State (a) the melting point of a mixture with x = 0.30, (b) the composition and proportion of the phases present when a solid of composition x = 0.30 is heated to 2200°C, (c) the temperature at which a liquid of composition y = 0.70 will begin to solidify.
Magnesium oxide and nickel oxide withstand high temperatures. However, they do melt when the temperature is high enough and the behavior of mixtures of the two is of considerable interest to the ceramics industry. Draw the temperature composition diagram for the system using the data below, where x is the mole fraction of MgO in the solid and y its mole fraction in the liquid. /C 1960 2200 2400 2600 2800 x 0 0.35 0.60 0.83 1.00 y 0 0.18 0.38 0.65 1.00 State (a) the melting point of a mixture with x = 0.30, (b) the composition and proportion of the phases present when a solid of composition x = 0.30 is heated to 2200C, (c) the temperature at which a liquid of composition y = 0.70 will begin to solidify.
define Gibb's rule and explain the relationship between Gibb's Free energy and the feasibility of reactions
A gas is confined to a subvolume v1 in an insulated rigid container. the container has an adjoining subvolume v2 initially evacuated which can be connected to v1 by opening the valve. if the valve is opened and the gas flows out of v1finally filling the entire volume v1+v2, calculate the work done by the gas in this expansion and change the internal energy of the gas
state the reasons why irradiation that produces excited electronic state alters the reactivity of some molecules
two reactions may have similar photochemical efficiencies but differ greatly in rate constant, briefly illustrate the theory
A mixture of gases is at equilibrium: 2 SO3 (g) → 2 SO2 (g) + O2 (g) ∆H = 197.78 kJ (a) Does the equilibrium shift to the left or to the right when some SO3 (g) is added to the reaction mixture? (b) Does the equilibrium shift to the left or to the right when some SO2 (g) is added to the reaction mixture? (c) In which direction does the equilibrium shift as the temperature is lowered? (d) In which direction does the equilibrium shift as pressure is applied to the system?
The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl (g) → 2 NO (g) + Cl2 (g) Suppose that 0.510 mol NOCl is placed in a 3.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of Cl2 is 0.0346 M. Calculate the equilibrium constant for this reaction
1)Consider the following reaction: N2O4 (g) → 2 NO2 (g) Assume that an experiment is carried out in which the starting concentration of N2O4 (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established, the concentration of NO2 (g) is 2.43 x 10-2 mol/L. Calculate the equilibrium constant for the above reaction.
2)Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.920 mol N2 and 0.700 mol O2 are mixed in a 3.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)
How many H atoms are present in 0.235 g of NH3?
