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Suppose that 50.0g of Zinc and 50.0g of Iodine are used to form Zinc (II) Iodide. Answer the following questions:
(A) What is the limiting reagent?
(B) How many grams of Zinc (II) Iodide can be produced?
(C) How many grams of excess element remain unreacted?
what is the pH of a solution obtained by adding 3.50g of HBr to 435mL of a 0.639M solution of HNO3?
Suppose that ammonia (a monoprotic base), applied to a field as a fertilizer, is washed into a farm pond containing 3.0 × 106 L of water. If the pH of this pond is found to be 9.81.
A sealed-end water manometer attached to an air duct reads 1598 cm. An open-end water manometer attached to the same duct reads 556.2 cm.
A 285- flask contains pure helium at a pressure of 750 . A second flask with a volume of 470 contains pure argon at a pressure of 716 .If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of h..
2 NO(g) + O2(g) 2 NO2(g) In one experiment 0.633 mole of NO is mixed with 0.354 mole of O2. Calculate also the number of moles of NO2 produced.
Determine what is the mass percent yield from 2.57 grams of Sb in excess Sulphur , if 1.56 g of Sb 2 S 3 is obtained?
0.74 L of a 0.41 M solution is diluted to a final volume of 3200 mL. What is the resultant molarity?
How many grams of sodium formate, NaCHO2, must be added to 750.0mL of .250 M of formic acid, HCHO2, to obtain a buffer with pH of 5.5
Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA
If 4.10 mol calcium carbide (CaC2) reacts with an excess of water, how many moles of acetylene (C2H2) will be produced?
If more than one alkene is possible, predict which one will be formed in the largest amount: a. 2-methyl-2-butanol b. 1-methylcyclohexanol
calculate the equilibrium constant from an absorbance value but my professor never told us how to calculate this.
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