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Problem- What is the experimental yield (in grams) of the solid product when the percent yield is 75.92 % when 1.180 g of silver nitrate reacts in solution with excess sodium phosphate?
AgNO3(aq) + Na3PO4(aq) --> Ag3PO4(s) + NaNO3(aq) [unbalanced]
Depict your all calculation in detail so I can understand the solution thoroughly
Classify each of the following molecules as polar or nonpolar: a) GeH4; b) I2; c) CF3Cl; d) PCl3; e) BCl3; f) SCl2.
Calculate the pH when 26.6 mL of 0.0025 M HCl is added to 100.0 mL of pure water. Comment and hint in the general feedback.
Calculate the concentration of iron (II) chloride contaminant in the original groundwater sample. Round your answer to significant digits.
Ammonia,NH3 ; ammonium nitrate,NH4NO3 ; and ammonium hydrogen phosphate (NH4)2HPO4, , are all common fertilizers. Rank the compounds in order from largest mass percent of nitrogen to smallest mass percent of nitrogen.
In chemical reactions the total number of moles of products must be the same as the total number of moles of reactants.
Problem- A certain gas is present in a 11.0L cylinder at 2.0atm pressure. If the pressure is increased to 4.0atm the volume of the gas decreases to 5.5L . Find the two constants ki, the initial value of k, and kf, the final value of k, to verify w..
A 4.80 g nugget of pure gold absorbed 298 J of heat. What was the final temperature of the gold if the initial temperature was 24.0°C? The specific heat of gold is 0.129 J/(g·°C).
The valence electrons of group 5A elemnts are in the 6s subshell. 8. The highest principle quantum number of period 2 elements is 2.
(a) Explain How many grams of N2(g) will be formed from 5.19 x 1022 molecules of CO(g) at STP. (b) Name each chemical.
Hydration of alkynes (via oxymercuration) gives good yields of single compounds only with symmetrical or terminal alkynes. Draw the major organic product(s) formed when hex-2-yne undergoes hydration
calculate the total volume of gases that can be collected at 1.2 atm and 293 k from 260 grams of nitroglycerin 4
Gaseous hydrogen iodide is placed in a closed container at 425 degree celcius, where it partially decomposes to hydrogen and idine: 2HI(g)--->--->H2(g)+I2(g). At equilibrium it is found that (HI)=3.53*10^-3 M,(H2)=4.79*10^-4M, and (I2)=4.79*10^-4M..
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