At 25°C methanol (CH4O) has a density of ~0.792 g/mL. If a reaction requires the chemist to use 644.50 moles of methanol, what volume will be required (in liters)? Use these atomic masses: C = 12.011 amu; H = 1.008 amu; O = 15.999 amu.

You are given a mixture of CuCO3 and CuO.  You place the mixture in a crucible and heat it to decompose the CuCO3 into CO2 gas and CuO.  You made sure that the CuCO3 had completely decomposed by constantly heating it, cooling it, and weighing it until the mass remains the same. Using the data below from the experiment, calculate the % CuCO3 in the original sample. Mass of empty crucible:  22.19 g Mass of crucible + sample before heating: 23.193 g Mass of crucible + sample at constant mass: 22.851 g   PLease show and create one solution map: i made this solution map, is it correct? 1.561g CO2 x (1mol CO2/44.01g CO2) x (1mol CrCO3/1mol CO2) x (112.01g CrCO3/1mol CrCO3)= 3.973g CrCO3 than, (3.973/25.422) x 100% = 15.63% 2.) A 12.622 g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as BaSO4.  If 11.957 g of BaSO4 are obtained in the analysis, what is the percentage of sulfur in the original compound? (Need help with this one too)

Part A 4. How many grams of silver nitrate must react to give 1.00 g of Ag? Cu(s)+2A£NO;(ag)→Cu(NO3)2 (aq)+2Ag(s) Express your answer with the appropriate units. HA μΑ MAGNO3 Value Units Submit Previous Answers Request Answer X Incorrect; Try Again Provide Feedback

Aspirin can be prepared from salicylic acid ( C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride ( C4H6O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C,H6O3 + C4HO3 → C3H3O4 + C2H3O2 What is the theoretical yield, in grams, of aspirin (C,H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.01 g of salicylic acid with 3.73 mL of acetic anhydride? Type answer:

Driving 1000 miles a month is not unusual for a short-distance commuter. If your vehicle gets 23.30 mpg, you would use approximately 42.92 gallons of gasoline every month. The unbalanced chemical equation for the reaction is   C8 H18 + O2 >>>>> CO2 + H2O  If gasoline is approximated as C8H18 (density = 0.703 g/mL), how many grams of carbon dioxide does your vehicle emit every month?

* 00 3. Alum [KAI(SO4)2XH20] is used in food preparation, dye fixation, and water purification. To prepare alum, aluminum is reacted with potassium hydroxide and the product with sulfuric acid. Upon cooling, alum crystallizes from the solution. (a) A 0.6809-g sample of alum is heated to drive off the waters of hydration, and the resulting KAI(SO 2 weighs 0.3706 g. Determine the value of x and the complete formula of alum. SI Value of x: Complete Formula: (b) When 0.7557 g of aluminum is used, 8.460 g of alum forms. What is the percent yield? % yield tiy #3 4. 5. 7. n O

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How many grams of A must have decomposed if 21.53 grams of Y are formed according to the reaction below? 5A → X + 3Y Assume that the molar mass of A is 35.00 g/mol, the molar mass of X is 100.00 g/mol, and the molar mass of Y is 25.00 g/mol.  Enter your answer with four significant figures. Do not enter the grams units, just the number.

How much LiI is produced when 350.0 g of HI reacts completely with LiOH, according to the equation HI + LiOH → H2O + LiI ? NOTE: To make grading easier with a computer, the answer needs to be a number without units. Example: 456; 456.123, etc.

Consider the following chemical reaction HCl (aq)  + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3     Determine the excess reactant   The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction   Determine the type of this chemical reaction