Silicon tetrachloride (SicI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(8) -> SIC4() In one reaction, 0.507 mole of SiCI4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SICI4 = 169.9 g/mol; MW CI = 35.453 g/mol A 36 grams B 72 grams 27 grams D 63 grams

Aqueous solutions of ammonia 1NH32 and bleach (active ingredient NaOCl) are sold as cleaning fluids, but bottles of both of them warn: “Never mix ammonia and bleach, as toxic gases may be produced.” One of the toxic gases that can be produced is chloroamine, NH2Cl.Another toxic gas that can be produced is nitrogen trichloride, NCl3. What is the oxidation number of N in nitrogen trichloride?

How many moles of HNO3 will be produced from the reaction of 41.5 g of NO, with excess water in the following chemical reaction? 3NO2(g) + H20 (1) → 2 HNO,(g) + NO(g)

00 S Nazza .01608 ·018302 3. (part a). You are given 0.104 g of a sample of KwFex(C₂O4)y(H₂O)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C₂04]²- in the sample. Please show all of your detailed calculations.

#25y of a 23% by mass magnesium chloride (MW= 95.21 g/mole) solution is reacted with 125.0 mL da125M solution of silver nitrate (MW= 169.87g/mole) determine the mass of silver chloride (MW = 143.32 p/mole) produced

In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation.   (b) Calculate the theoretical yield of NaF.   (c) If 0.792 g of NaF is formed, calculate the percent yield.

For the reaction represented by the equation SO3+H2O-->H22SO4 how many grams of sulfuric acid (H22SO4) can be produced from 197 g of water and 460g of sulfer trioxide?

6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles

Based on the balanced reaction: 6 CO2 + 6 H2O→ 6 O2 + C6H12O6, what is the maximum number of grams of C6H12O6 that could be made by the reaction of (5.88x10^1) g of CO2 and excess water?

Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21