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2KClO3 -----> 2KCl + 3O2 so 2 moles produces 3 moles. 5 x 10-2 therefore produces :
5 x 10-2 x 3/2 = 7.5 x 10-2 moles. I mole of a gas occupies 22.4 liters at STP so:
7.5 x 10-2 x 22.4 = 1.68 liters.
Wiki User
∙ 11y ago
Wiki User
∙ 12y agoThe equation is represented as for figuring moles of O2 produces is as follows:
5g KClO3 * mol KClO3 * 3 mol O2 = 50 moles O2
122.55g KCLO3 2 mol KClO3 817
Now that we know the number of moles, we can use the ideal gas equation to solve for the volume:
PV=nRT
At STP, P= 1 ATM, and T= 0 degrees Celsius/273.15 K
The gas constant, R= 0.082057 L*ATM/mol*K
1 ATM * V Liters = (50/817) mol * 273.15 K * 0.082057 L*ATM/mol*K
V= approx. 1.37172
Wiki User
∙ 6y ago2KClO3 ==> 2KCl + 3O2 balanced equation for decomposition of KClO35 moles KClO3 x 2 moles KCl/2 moles KClO3 = 5 moles KCl
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What volume in milliliters will 0.00919 g H2 gas occupy at STP?
The volume is 102 mL.
How do you calculate the volume in milliliters of a 0.61M sodium nitrate solution that contains 400mmol of sodium nitrate?
By definition, a 0.61M sodium nitrate solution contains 0.61 moles of sodium nitrate per liter, which is equivalent to 0.61 mmol/ml. Therefore, the volume of this solution required to contain 400mmol is 400/0.61 or 6.6 X 102 ml, to the justified number of significant digits.
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?
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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
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 volume in milliliters will 0.00919 g H2 gas occupy at STP?
The volume is 102 mL.
What year was the daisy model 102 made?
The 102 cub was made between 1952-78
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
What chapter does fruits basket book 18 start with?
Volume 18 starts with chapter 102. (The last chapter in the volume is 107.)
