* Question Completion Status: QUESTION 14 In an experiment, a student obtained the following masses for a product: 0.651 g. 0.643 g. 0.648 g, 0.609 g, and 0.646 g. What is the average deviation from the mean? O 0.6394 g O 3.12 g O 0.0608 g O 0.012 g
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- When working in a lab over the holidays you find a vial of blue powder. The label is unintelligible, and the only thing can read is:Substance: Co(CX)6Moles: 0.0189molYou weigh the sample:Grams: 4.29gWhat is the compound? (Hint: what is X?)a hydrated CuSO4 salt was heated and thus dehydrated. Determine the % H2O by weight in the hydrated CuSO4 salt. SHOW WORK TO RECEIVE FULL CREDIT mass of empty dish 43.571 gmass of dish + hydrated salt 44.326 gmass of dish + dehydrated salt 44.054 g 4. Using the data found in question number 3, determine the empirical formula for the hydrated CuSO4salt. What is the chemical name of this dehydrated salt? 5. Suppose that after your second heating, you were impatient and did not wait until your porcelain evaporating dish to cool. Instead, you weighed it while it was still hot. How would this specifically affect the calculated percentage of water in the compound?Assume that the mass of impure acetanilide is 2.229 g. And the mass of recrystallized acetanilide is 1.225 g. Calculate the percent recovery. 2 decimals in answer with units.
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- The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 161 g of ammonia consumes __________ g of oxygen. atomic weights: N = 14.01, H = 1.01, O = 15.99. Input values only with two decimal places. Do not include the units.Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) COCl2(g) + Cl2(g), Kc = 4.4 × 109 at 1,000 KCalculate Kc for the reaction 2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g). Round off the answer to two significant digits. Group of answer choices 4.4 × 109 8.8 × 109 1.9 × 1010 1.9 × 1019 2.3 × 10–10How many moles are present in the 5.00 g of sodium bicarbonate you used for this experiment? n= 5.00/84.007 = 0.060 moles 2.4 How many moles of gas would be produced if this amount of sodium bicarbonate reacted completely with acetic acid, which you added as vinegar? What volume would this amount of gas occupy at room temperature (25.0 °C)? At refrigerator temperatures (4.0 °C)? Or at freezer temperature (−20.0 °C)? PV=nRT V= (nRT)/P V= n How many moles and grams of acetic acid would be required if 00 g of sodium bicarbonate reacted completely with no unreacted acid or base (i.e. with an exact stoichiometric ratio)?
- convert 1. 0.7 pg into ng 2. 13 dm to mm 3. 2.5x10-15 mole into pmole 4. 3.5 x105μm into cm 5. 50.0000 km/h into m/s 6. 50.0000 μg/ml into g/L 7.. 26.30 μmole/mL into mole/Lsolve for the gravemetric factor of the following: 1. Substance weighed: Mg(C9H6O2)2 & Substance sought: MgSO4 2. Substance weighed: HgI2 & Substance sought: HgO 3. Substance weighed: (NH4)2SO4 & Substance sought: NH3Number of molecules in 9×10−6 molmol CH3CH2OHCH3CH2OH. Express your answer using four significant figures