ClFx is an interhalogen compound which is known to be very irritant and toxic. These compounds are commonly used as rocket fuel and in the semiconductor industry. ClFx can be neutralized by reacting it with uranium to produce uranium hexafluoride and chlorine fluoride. The reaction of the compound with some uranium yields 5.63 grams of uranium hexafluoride and 457 ml of chlorine fluoride at 75oC and a pressure of 3.00 atm a). Find X! b).Determine the hybridization and molecular geometry of the compound!

Ozone 1O32 is formed in the earth’s upper atmosphere by the action of solar radiation on oxygen molecules 1O22. Write a balanced equation for the formation of ozone from oxygen.

The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN,) into solid sodium and gaseous dinitrogen. alb Ar 2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of 13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Accessibility <. lenovo dle WebEx at 3pm (dia' just before 3pm) Resp L-650-479-3208 Access Code (meeting Number): 737 129 915 Dois, 3134

2. A. Write a balanced chemical equation for the reaction, in aqueous solution, between silver nitrate and sodium bromide. A fine pale yellow precipitate is observed from this mixture. Which compound is the precipitate? B. How many moles of air are present in the lungs if they occupy a volume of 5.0 L at 37°C and 725 mmHg? How many molecules of air is this?

b If [OH ] 2.9 x 10¬10 M then РОН

The habor process is the production of ammonia from gaseous nitrogen and hydrongen. how many grams of nitrogen gas are required to produce 10.00g of ammonia, assuming a 75% yield and excess hydrogen gas?

Mass→Mass & Mass→Vol : Zinc citrate is used in toothpaste it is synthesized from zinc carbonate and citric acid according to the following reaction. A) What mass of Zn₃(C₆H₅O₇)₂ can be produced from 2240. g of ZnCO₃? B) How many L of CO₂ will be produced at STP by this amount?

Sodium hydrogen sulfate is used as a cleaning agent and as a flux (a substance that promotes the fusing of metals and prevents the formation of oxides). One of the ways in which sodium hydrogen sulfate is manufactured is by reacting sodium dichromate, Na2Cr2O7, with sulfuric acid. This process also forms water and chromium(VI) oxide, CrO3. Write a balanced equation for this reaction. (You do not need to include states.) How many kilograms of sodium dichromate, Na2Cr2O7, are necessary to produce 130.4 kg of sodium hydrogen sulfate? How many kilograms of chromium(VI) oxide are formed when 130.4 kg of sodium hydrogen sulfate is made? What is the minimum volume of 18.0 M H2SO4 solution necessary to react with 874.0 kg of sodium dichromate? What is the maximum mass of sodium hydrogen sulfate, NaHSO4, that can be formed from the reaction of 874.0 kg of sodium dichromate with 400.0 L of 18.0 M H2SO4?

Mass of copper before electrolysis 5.621 g Mass of copper after electrolysis 5.487 g Volume of H2 collected 53.6 mL Pressure of H2, PH2 727.0 mm Hg Temperature 21.3 oC 1. Determine and report the pressure of collected hydrogen gas in atmospheres. Report this result to one more digit than allowed by applying the rules of significant figures. (1 atm = 760 mm Hg, an exact conversion factor.) 2. Determine the moles of hydrogen collected by substituting the appropriate quantities into the ideal gas equation and solving. Report this result to one more digit than allowed by applying the rules of significant figures. Notes: the gas temperature is the same as the listed temperature; R = 0.082057 L-atm/mol-K. Be mindful of units. 3. Determine the experimental atomic mass of Cu. Round this result to the correct number of significant figures. 4. Determine the percent relative error (= ????????????−?ℎ????????? ?ℎ????????? ? 100). The molar mass of Cu is 63.546 g/mol.

The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN) into solid sodium and gaseous dinitrogen. dlo 2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of 13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy | Accessibility > Activity Details You have viewed this topic MacBook Air 4) DI DD F10 F11 F9 F2 F3 F4 F1 10 #3 $ & 3. 4. 6. 8 9.