calculate the mase of KClO3 that could be used to produce 0.0193 moles of oxygen ?
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s) . The equation for the reaction is 2KClO3⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 70.4 g KClO3(s) STRATEGY: Convert the mass of KClO3 to moles. Convert the number of moles of KClO3 to the number of moles of O2 . Convert the number of moles of O2 to grams. Step 1: 70.4 g KClO3 is equal to 0.574 mol KClO3...
Solid potassium chlorate (KClO3) decomposes into potassium chloride and oxygen gas when heated. How many moles of oxygen form when 55.3 g completely decomposes? 0.338 mol 0.677 mol 0.451 mol 83.0 mol
The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory 2KCIO3 (8) ► 2KCI (s) + 302 (9) What volume (L) of O2 gas at 25°C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO3 (s)? Select one: a. 11 b.4.5 CO d. 3.7 e. 2.3
You are given an unknown containing KClO3. Following the procedure in your manual, you obtain the following fictional data Note! For this problem use the given (allbeit incorrect) vapor pressure of water Mass of empty test tube 71.8394 g Mass of test tube + unknown 72.1363 g Mass of test tube + unknown + MnO2 72.3077 g Mass of erlenmeyer flask with residual water 323.06 g Mass of erlenmeyer flask filled with water 358.52 g Atmospheric pressure 760.9 mmHg Temperature...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The equation for the reaction is 2KClO3⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 98.6 g KClO3(s). mass:
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The equation for the reaction is 2KClO3⟶2KCl+3O2⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 48.8 g KClO3(s).
Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) ? 3 CO2(g) + SO2(g) + 4 H2O(g) 6.21 moles O2 3.50 moles O2 4.14 moles O2 2.33 moles O2 1.55 moles O2
5.0 moles of iron reacts with 5.0 moles of oxygen gas to produce iron(ll)poxide. What is the Limiting Reagent? ronlI)oxide Iron Oxygen Question 2 (1 point) How many moles of iron(ii)oxide are formed (enter the answer without units and use correct number of significant figures)?
Consider the following reaction. How many moles of oxygen are required to produce 6.00 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)
Calculate the moles of oxygen needed to react with 7.500 moles of benzene by combu Number moles of oxygen Previous Give Up & View Solution Check Answer ON MacBook Air of F2 2013 og