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1. Calculate the final pressure in atm while using a sample of helium gas that was initially at 785 torr , 37.0°C, and 1.00 L was heated to 68.0°C while the volume expanded to 3.24 L. ?
2. Calculate the rate constant for the reaction when the reactant concentration in a first-order reaction is given 7.30×10-2M after 15.0s and it is also reported 4.40×10-3M after 65.0s . ?
Determine the molar concentration of chloride ions after adding 225 ml of 0.625 MKCL with 615 ml of 0.385M MgCl2 if final volume of the solution is 840ml.
Find the mass of the substance and the volume of a gas in a reaction - determine the mass of solid ammonium nitrate that must be used to obtain 0.145 L of dinitrogen oxide gas at STP.
Determine the concentration of a solution prepared by diluting 25.0 milliliters of a 12 molar HCl solution with H2O until the final volume is 2.50 x 10² milliliters.
The _______ of a titration occurs when the indicator changes color.
Find the theoretical, percent yield and percent error of the reaction - Calculate the percent error of this reaction.
Identifying and balancing the different types of chemical reactions. Evaluate which processes represent chemical reactions.
To calculate the number of molecules of a gas using ideal gas law and Avogadro's number - How many ozone molecules are present in 1.0 L of air under these conditions?
Explain the structural feature of Acetanilide molecule - Identify one structural feature of the acetanilide molecule
3H2 (g) + N2 (g) 2NH3(g), Kc = 6.0 × 10-2 at 500°C for this nitrogen fixation reaction. What is the equilibrium concentration of N2 If 0.250 M H2 and 0.050 M NH3 are present at equilibrium?
Write the nuclear equation for the alpha decay ( production of radioactive decay that may be considered radioactive waste products by the useful production of nuclear energy ) of each nuclide that are products of a nuclear power plant Rn-222, T..
Find the lowest temperature of vaporization and the highest temperature when there is liquid left over and Determine the range of temperatures which could be used for this process.
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Compute the pH of the solution before the addition of any HNO3. Kb of NH3 =1.8 × 10-5.
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