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How many moles of O2 are needed to to produce 10.2 moles of H2O?
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How many moles of aluminum oxide are present in a sample having a mass of 178.43g?
For this you need the atomic (molecular) mass of Al2O3. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. Al2O3= 102 grams408 grams Al / (102 grams) = 4.00 moles Al
What is the molarity of a 2.50 x 102 cm3 solution containing 45.0 g of C6H12O6?
Molarity is defined as moles solute/liter of solution.Moles of solute = 2.5 moles sucrose Liters of solution = 0.5 liters Molarity (M) = 2.5 moles/0.5 liters = 5 M
How many moles of carbon dioxide are produced when 10 moles of propane are combusted?
This question sound like one that can easily be answered if one has a general chemistry textbook. My advice is to look at doing some unit conversions to find out how many moles of propane are in 36.1 g of propane first. With a balanced chemical equation for combustion, and assuming the propane is the limiting reagent, use dimensional analysis to convert your moles of propane to moles of carbon dioxide.
How do you calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen?
Aluminum Oxide is Al2O3 and Al = 27 and oxygen =16 so the molar mass is 102 g/mol Al2O33.75 mol Al ~ 3.75/2 mol Al2O3 ~ (3.75/2)mol * 102 g/mol = 191.25 = 191 gram Al2O3
What is the theoretical yield of aluminum oxide if 2.40 mole of aluminum metal is exposed to 2.10 mol of oxygen?
Balanced equation: 4Al(s) + 3O2(g) ==> 2Al2O3(s)2.40 mol Al ==> 1.2 moles Al2O3 (mole ratio of Al2O3 : Al is 2:4 or 1:2)2.10 mol O2 ==> 1.4 moles Al2O3 (mole ratio of Al2O3:O2 is 2:3)Therefore, Al is the limiting reactant.Theoretical yield will thus be 1.2 moles Al2O3. If you need mass, it is 1.2 moles x 102 g/mol = 122 g
If a chemistry student collected 856 mL of gas at 25C and 7.40 102 torr how many moles did she collect?
0.0341
If a chemistry student collected 825 mL of gas at 25ºC and 7.90 102 torr how many moles did she collect?
0.0351
If a chemistry student collected 856 mL of gas at 25.0ºC and 7.40 102 torr how many moles did she collect?
0.0341
If a chemistry student collected 834 mL of gas at 25ºC and 8.00 102 torr how many moles did she collect?
0.0359
If a chemistry student collected 834 mL of gas at 25ºC and 8.00 × 102 torr, how many moles did she collect?
0.0359
If a chemistry student collected 834 mL of gas at 25C and 8.00 x 102 torr how many moles did she collect?
0.0359
If a chemistry student collected 825 mL of gas at 25 C and 7.90 102 torr how many moles did she collect?
0.0351
4.32 x 102 moles of CH3COOH in 20.0 liters of water?
21.6
If liquid carbon disulfide reacts with 4.50 x 102 mL of oxygen to produce the gasses carbon dioxide and sulfur dioxide what volume of each product is produced?
First, write out your balanced equation. CS2 (l) + 3O2 (g) → CO2 (g) + 2SO2 (g) Then, since you know by Avogadro's Law, the volume is directly proportional to the number of moles. Since 3 moles of oxygen gas form one mole of carbon dioxide, you divide 4.50 x 102 mL, or 450. mL, and you get 150. mL of CO2 (g). Since 3 moles of oxygen produce 2 moles of sulfur dioxide, you take 450. mL and multiply it by (3/2) and get 300. mL of SO2 (g).
What is the prime factorization of 102 exponent form?
It is: 2*3*17 =102 and exponents not needed
How many moles of nitrogen are in 4.0 times 10 with the power of 2 of quinine?
The clarity of this question is not clear. I will assume grams and possibly moles as that number does not look like a number of atoms. Grams first, then moles. 4.0 X 102 grams quinine (1 moleC20H2N2O2/302.236 grams)(2 moles N/1 mole C20H2N2O2) = 2.6 moles nitrogen =============== Pretty much the same procedure if you meant moles just no dividing out a mass.
How many moles of aluminum oxide are present in a sample having a mass of 178.43g?
For this you need the atomic (molecular) mass of Al2O3. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. Al2O3= 102 grams408 grams Al / (102 grams) = 4.00 moles Al
