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- Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C4H10(g) + 13 02(g) - 8 CO2(g) + 10 H20(g) X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 10 126 2 13 2.18 1 8 6.022 x 1023 18.02 0.0374 4.35 8.70 44.01 58.14 208.00 g O2 g C4H10 g H20 mol H20 g CO2 mol CO2 mol O2 mol C4H10X in the following equation is a value of * COOH .6. + X 0₂ Your answer true One of the products of the reaction of one mole of sodium hypochlorite with two moles of ammonia is the formation of chloroamine Error OH -6 true + ? CO₂ Atmospheric air is one of the most important sources for the preparation of industrial gas (hydrogen + carbon .monoxide) Error * *What is the gravimetric factor when the desired substance is Cr2O3 and the weighed substance is PbCrO4? 1 mole Cr2O3 is to 3 moles PbCrO4 1 mole Cr2O3 is to 2 moles PbCrO4 2 moles Cr2O3 is to 1 mole PbCrO4 2 moles Cr2O3 is to 2 moles PbCrO4
- How many moles of O2 will be formed from 2.00 moles of KCIO, for the following reaction? Answer to 2 decimal places. The unit for mole is mol. 2 KCIO3→ 2 KCI + 3 O2 Your Answer: Answer unitsSTARTING AMOUNT esc X How many moles of Na₂SO are in a 0.140 m aqueous solution that was prepared with 2.30 kg of water ? ADD FACTOR x( ) 0.140 6.022 x 1023 mol Na₂SO 0.322 1 g water 609 2.30 kg water ANSWER 142.04 45.7 kg Na₂SO 322 g Na₂SO RESET 2 0.609Answer 1.2x10-3 moles AgBr
- Macmillan Learning Suppose you performed a reaction between aqueous copper(II) chloride, CuCl₂, and solid iron, Fe, in the lab. When you added 0.976 g of Fe to 18.2 mL of 0.143 M CuCl₂, you observed that the solution changed in color from turquoise blue to yellow/brown with iron remaining in the solution. Identify the limiting reagent. CuCl₂ and Fe are in equal amounts O cannot be determined 0 Fe Q CuChSTARTING AMOUNT esc + 30 F1 X F2 80 F3 2 What quantity of moles of Care formed upon complete reaction of according to the generic chemical reaction: ADD FACTOR X 0.500 6.022 x 1023 000 000 F4 F5 1 mol B A + 2 2 1.20 x 1023 mol A B-C N F6 MacBook Air ANSWER 4 mol C F7 8 DII F8 mol of B RESET 5 3.01 x 1023 DD F9 F10 (4) F11 CQuestion 1 of 8 Submit Calculate the theoretical yield in grams All: from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: Al(s) + :(s) – 2 All:(s) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 3 138 1 18.3 0.678 1.47 407.7 277 26.98 mol Alls g/mol Alls mol Al g/mol Al g Alls g Al 2.
- Using this balanced equation: NaHCO3 + CH3COOH H2O + CO2 + NaC2H3O2 In an experiment , the following mass measured 3.0 grams, 5.5 grams and 7.0 grams of Baking soda is mixed with 0.5 mol of acetic acid (vinegar) to form carbon dioxide as a product formed Name of Bottle NaHCO3 (Baking Soda) Acetic Acid Calculation of Amount of Product Formed Mass Mole Volume Mole Limiting Excess A 3.0 g 50 mL 0.5 mol B 5.5 g 50 mL 0.5 mol C 7.0 g 50 mL 0.5 molIn respiration process, one molecule of C6 H12O6 reacts with oxygen and produces water and CO2. Now, a healthy person needs 390 ml oxygen per minutes and he respires 13 times per minute. So, what is the amount of CO2 he exhales per respiration (in ml)?Activity 2. Perform the needed calculations for the problem and show your complete calculations in a clean sheet of paper. Box your final answer. 1.Metabolic breakdown happens when glucose (C6H12O6) is reacted with oxygen gas O2(g) forming carbon dioxide (CO2) and water (H2O) as shown by the equation below: C6H1206 (s) + 602{g) 6CO2(g) +6 H2O (1) Determine the volume of CO2 produced at 37 °C and 1.00 atm when 5.60 g of glucose is used up in the reaction. Molar mass: Glucose=180.15 g/mol 2. Calculate the mass in grams of hydrogen chloride produced when 5.6 L of molecular hydrogen (H2) measured at STP react with an excess of molecular chlorine gas Cl2(g).