Question

How many mL of 0.122 M MnO4 - are required to react with an excess of...

How many mL of 0.122 M MnO4 - are required to react with an excess of C2O4 2- in order to produce 75.25 mL of carbon dioxide gas measured at 30.0 C and 715 Torr?

MnO4 - (aq) + C2O4 2- (aq) --> MnO2 (s) + CO2 (g) (basic solution)

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A.) FeCl2 is water soluble. what ions are formed when this compound dissolves in water? B.)...
A.) FeCl2 is water soluble. what ions are formed when this compound dissolves in water? B.) If the solution is 0.255 M FeCl2 what is the molarity of each ion in aqueous solution? C.) Find the percentage of FeCl2 in a 35.5g sample of ore which has been dissolved in aqueous acid and titrated to the endpoint with 23.55 ml of 0.309 M Cr2O7^2- . the molar mass of FeCl2 is 126.0 g/mol. Cr2O7^2- + Fe^2+ ------> Cr^3+ + Fe^3+...
A 20.00 mL sample of MnO4 is required to titrate .2378 g Na2C2O4 in an acidic...
A 20.00 mL sample of MnO4 is required to titrate .2378 g Na2C2O4 in an acidic solution. How many mL of this same MnO4 -1 are required to titrate a 25.00mL sample of 0.1010 M Fe+2 in acidic solution [ 5 pts] Eq 1: 2 MnO4 -1 (aq) + 16 H+1 (aq) + 5 C2O4 -2 (aq) → 2 Mn +2 (aq) + 8 H2O (l) + 10 CO2 (g)
How many liters of carbon dioxide gas, measured at 20 degrees Celsius and 715 torr, are...
How many liters of carbon dioxide gas, measured at 20 degrees Celsius and 715 torr, are formed when 49 grams of chalk (CACO3, 100.9 g/mol) are reacted with 60 ml of 3.20 M sulfuric acid (H2SO4) according to the following molecular equation (R= .0821 Latm/molK). CACO3 (s) + H2SO4 (aq) -> CO2 + H2O (l) + CASO4 (s)
37.3 mL of a 0.129 M Na2CO3 solution completely react with a 0.150 M HNO3 solution...
37.3 mL of a 0.129 M Na2CO3 solution completely react with a 0.150 M HNO3 solution according to the following balanced chemical equation: Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l) What mass (in grams) of carbon dioxide is formed?
In the following chemical reaction, how many moles of O2 are needed to produce 2.8 mol...
In the following chemical reaction, how many moles of O2 are needed to produce 2.8 mol of CO2? C2H6 + O2 → CO2 + H2O? How many moles of methane are produced when 36.6 moles of carbon dioxide gas react with excess hydrogen gas? How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor? Plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen in the process...
1) What is the density (in mg/mL) of a H2S gas at 12.9 atm and 137...
1) What is the density (in mg/mL) of a H2S gas at 12.9 atm and 137 K? 2) Calcium carbonate reacts with hydrochloric acid to produce carbon dioxide gas. If 35.3 g of calcium carbonate reacts with 100 mL of 6.00 M HCl, how many liters of carbon dioxide gas will be produced at 745 mmHg and 23.0 °C? (Hint: Limiting Reactant) CaCO3 (s) + HCl (aq)  →  CaCl2 (aq) + CO2 (g) + H2O (l)   (unbalanced)
1) How many grams of Ag2CO3 will precipitate when excess K2CO3 solution is added to 53.0...
1) How many grams of Ag2CO3 will precipitate when excess K2CO3 solution is added to 53.0 mL of 0.713 M AgNO3 solution? 2AgNO3(aq) + K2CO3(aq) = Ag2CO3(s) + 2KNO3(aq) ?g 2)How many mL of 0.695 M HBr are needed to dissolve 8.81 g of MgCO3? 2HBr(aq) + MgCO3(s) = MgBr2(aq) + H2O(l) + CO2(g) ? mL
A solution of permanganate is standardized by titration with oxalic acid (H2C2O4). It required 28.97 mL...
A solution of permanganate is standardized by titration with oxalic acid (H2C2O4). It required 28.97 mL of the permanga- nate solution to react completely with 0.1058 g of oxalic acid. The unbalanced equation for the reaction is MnO4- (aq) + H2C2O4(aq) ----> Mn^2+ (aq) + CO2(g) What is the molarity of the permanganate solution?
A 61.0 mL sample of a 0.122 M potassium sulfate solution is mixed with 34.5 mL...
A 61.0 mL sample of a 0.122 M potassium sulfate solution is mixed with 34.5 mL of a 0.120 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 0.999 g . Determine the theoretical yield (mass of PbSO4) , and the percent yield.
1a. How many moles of carbon monoxide are required to react completely with 3.38 L of...
1a. How many moles of carbon monoxide are required to react completely with 3.38 L of oxygen gas according to the following reaction at 0°C and 1 atm? carbon monoxide (g) + oxygen(g)carbon dioxide (g) ____________ moles carbon monoxide? 1b. What volume of hydrogen gas is required to react completely with 1.21 mol of nitrogen gas according to the following reaction at 0°C and 1 atm? nitrogen (g) + hydrogen(g)ammonia (g) ______________liters hydrogen gas?