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In the laboratory, you are studying the first-order conversion of a reactant to products in a reaction vessel with a constant volume of . At 1:00 p.m., you start the reaction at 21 with 1.000 of . At 2:00 p.m., you find that 0.600 of remains, and you immediately increase the temperature of the reaction mixture to 31. At 3:00 p.m., you discover that 0.250 of is still present. You want to finish the reaction by 4:00 p.m. but need to continue it until only 0.040 of remains, so you decide to increase the temperature once again. What is the minimum temperature required to convert all but 0.040 of to products by 4:00 p.m.?
There are very few compounds that contain an element from the noble gas family (elements in column 18, rightmost column). Explain why there are so few noble gas compounds in nature.
Up to Iron "Fe", the number of proton and neutron are about equal, after Fe the number of neutron began to rapidly increase, with respect to the number of proton, why?
if 2.29 moles of argon gas are added to 3.5L of a 6.58 mole sample of argon gas what is the final volume
At 25 c and 1.0 atm, 0.25 g of a gas dissolves in 1.00 L of water. What mass of the gas dissolves in 1.00 L of water at 25 c and 3.0 atm?
It then gives off a photon having a wavelength of 1740 nm. What is the final state of the hydrogen atom? Values for physical constants can be found here.
In fermentation of glucose, 780 mL of CO2 gas was produced at 37 degrees C and 1.00 atm. What is the volume(L) of the gas when measured at 22 degrees C and 675 mmHg?
Titration of sodium carbonate with HCl to the methyl orange end point involves the reaction of 1 mole of Na2CO3 with 2 moles of HCl. Write the balanced chemical equation in a.
Titrations: Finding Mass Percent of Arsenic in a Pesticide, The arsenic in a 1.0211-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized and exactly 40.00 mL of 0.05922M
find the number of moles of water that can be formed if you have 218 moles of hydrogen gas and 104 moles of oxygen gas
The air pollutant NO is produced in automobile engines because of the high-temperature reaction below. If the initial concentrations of N2 and O2 at 1000 K are both 1 M
how many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3+6NO-- 5N2+6H2O
Determine how many grams of solute would separate if the quantity of the solvent is 129 grams if a saturated solution of ammonium nitrate at 75 °C is cooled to fifteen degree Celsius?
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