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Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is 7.1x10^-7. a.) 0.065 M Ca(NO3)2 b.) 0.065 M NaIO3
A gas occupies 10.0 L at 44.1 psi and 27 degrees C. What volume will it occupy at standard conditions
the heat change value that you calculate from your experiments will be for the amount of material that you use in each reaction. how will you convert it to kJ/mol
write a general equation that illustrates all acid-base reactions. using equation, what factor can be varied to observe their effect on HEAT
What conditions are used in the Haber process to enhance the yield of ammonia. Explain why each condition affects the yield in terms of the Le Chatelier principle
Which atom has the largest partial positive charge in these bonds. C-H, C-O, C-F, C-Cl C in C-O Cl in C-Cl O in C-O F in C-H C in C-H C in C-Cl C in C-F
Out of what will you construct your calorimeters? please answers have to be related to chemistry and specifically to this experiment.
you will need to construct a calorimeter to complete this project. what are the necessary features of a calorimeters. please answers have to be related to chemistry and specifically to this experime
what are the goals of this project. please answers have to be related to chemistry and specifically to this experiment.
For the following, identify the process as a spontaneous process, a nonspontaneous process, or an equilibrium process at the specified temperature.
What mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each of the following pH values pH = 2.70? pH = 1.70? pH = 0.60
Calculate the pH and pOH of each of the following solutions. [H3O+] = 1.5x10^-8 M? [H3O+] = 1.0x10^-7 M? [H3O+] = 2.2x10^-6 M
At 800K the equlibrium constant, Kp for the following reaction is 3.2 *10^-7. 2H2S(g)<---->2H2(g)+S2(g). A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allow
Write a chemical equation for HF(aq) showing how it is an acid or a base according to the Arrhenius definition. Write a chemical equation for Ba(OH)2(aq) showing how it is an acid or a base accordin
How many moles of H3O+ must be added to one liter of a solution to adjust the pH from 8.54 to 5.58? Use E notation and 3 significant figures.
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
Calculating the Heat of Reaction from Heats of formation Use the following information to find ^Hf of methanol [CH3OH(l)]. CH3OH(l) + 3/2 O2(g) CO2(g) + 2 H2O(g) (heat)H°
Acetylene burns in air according to the following equation. C2H2(g) + 5/2 O2(g) 2 CO2(g) + H2O(g) H0rxn = -1255.8 kJ Given that H0f of CO2(g) = -393.5 kJ/mol and H0f of H2O(g) = -241.8 kJ/mol, what
Using Hess's Law to Calculate an Unknown heat ^ H Nitrogen oxides undergo many interesting reactions in the environment and in industry. Given the following information, calculate H for the overall
Calculate Hrxn for the reaction below. Ca(s) + 1/2 O2(g) + CO2(g) CaCO3(s) You are given the following set of reactions. Ca(s) + 1/2 O2(g) CaO(s) H = -635.1 kJ CaCO3(s) CaO(s) + CO2(g) H = 178.3 kJ
Using the Heat of Reaction (Hrxn) to Find Amounts Organic hydrogenation reactions, in which H2 and an "unsaturated" organic compound combine, are used in the food
A mercury mirror forms inside a test tube by the thermal decomposition of mercury(II) oxide. 2 HgO(s) 2 Hg(l) + O2(g) Hrxn = 181.6 kJ (a) How much heat is needed to decompose 504 g of the oxide? kJ
Consider the reaction Cl2(g) + I2(g) <=> 2 ICl(g), which is endothermic as written. What would be the effect on the equilibrium position of increasing the volume of the reaction container
Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are
When 26.0 mL of 0.565 M H2SO4 is added to 26.0 mL of 1.13 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and K