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Phosphorus pentachloride is used in the industrial preparation of organic phosphorus compounds. Equation 1 shows its preparation from PCl3 and Cl2. (1) PCl3(l) + Cl2(g) PCl5(s) Use equations 2 and 3 to calculate ?H°rxn of equation 1. (2) P4(s) + 6 Cl2(g) 4 PCl3(l) ?H = -1280 kJ (3) P4(s) + 10 Cl2(g) 4 PCl5(s) ?H = -1774 kJ
A 2.50-g sample of a large biomolecule was dissolved in 37.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C.
Determine the volume of the gas at a pressure of 150.0 kPa and a 26 degree Celsius of temperature?
A gaseous compound is 78.14 percent boron and 21 86 percent hydrogen . At 27 degrees celcius, 74.3 ml of gas exerted a pressure of 1.12 atm.
A sample of gas is stored in 716 mL tank at 205 kPa and 300 K. The gas is transferred to a different tank with a volume of 925 mL and 325 K. What is the pressure of the gas in the second tank?
An experiment requires 45.8 g of ethylene glycol, a liquid whose density is 1.114 g/mL. Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder.
Compute the value of ΔH ° if the combustion products are CO2 (g) and H2O (g). it isgiven that: CO 2 (g) = ΔHf ° - 393.5 kJmol-1; H 2 O (l) = ΔHf ° -285.8 kJmol-1; H 2 O (g) = ΔHf ° -241.8 kJmol -1.
Calculate the values of q, w, delta U, and delta H for the reversible adiabatic expansion of 1 mole of a monatomic ideal gas from 5.00 m^3
Imidazole is a weak acid, and thus reacts with strong bases to form the corresponding anion. Show this reaction, and draw resonance structures that account for the stability of conjugate base.
Find the empirical formulas for compounds with the following compositions: a. 8.74% magnesium, 91.26% iodine b. 36.86% nitrogen, 63.14% oxygen
How many moles of oxygen atoms are combined with 4.20 moles of chlorine atoms in Cl2O7?
calculate the activation energy for diffusion for a system where the diffusion coefficient doubles its value from 700k to 1200k. R=8.314J/molk.
Consider a molecule with spacing between two energy levels of 0.250 kJ mol-1. Calculate the wavelength and wavenumber of the photon that would be needed to lead to an excitation between these two levels.
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