Dr. Furst stoich test 1

2MnO4- (aq) +5 C2O42- (aq) + 16 H+ (aq) → 2Mn2+ (aq) +10 CO2(g) + 8 H2O (l) permanganate and oxalate ions react in and acidified solution according to the balanced equation above how many moles of CO2(g) are produced when 20. ml of acidified 0.20 M KMnO4 solution is added to 50. ml of 0.10 M Na2C2O4 solution

0.010

A 0.20 mol sample of MgCl2 and a 0.10 mol sample of KCl are dissolved in water and diluted to 500 ml what is the concentration of Cl- in the solution

1

for the reaction 2S +3 O2 → 2 SO3 how much SO3 can be produced from 7.08 g O2 and excess S

11.8

. . . C10H12O4S(s) + . . . O2(g) → . . . CO2(g) + . . . SO2(g) + . . . H2O(g) When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2(g) is

12

Au2 S3 + 3 H2 → 3 H2 S + 2 Au What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2

19.7

LiHCO(aq) +H2SO4(aq) → LiSO4(aq) + H2O(l) + CO2(g) when the equation above is balanced and the coefficients are reduced to the lowest whole number terms what is the coefficient of H2O(l)

2

C3H8(g) + 5 O2 (g) <-----> 3 CO2 (g) + 4 H2O (l) In the reaction represented above what is the total number of moles of reactants consumed when 1.00 mole of CO2(g) is produced

2.00

What volume of solvent should be added to 36.8 g of CH3OH to produce a 0.500 M solution of CH3OH

2.30

H2+ F2 → 2HF In the Reaction represented above what mass of HF is produced by the reaction of 3e1023 molecules of H2 with excess F2

20.

Li3N(s) + 2 H2(g) → LiNH2 (s) + 2 Li H(s) Because pure H2 is a hazardous substance safer and more cost-effective techniques to store it as solid for shipping purposes have been developed one such method is the reaction represented above which occurs at 200 degrees Celcius when 70.35 g Li3N(s) reacts with excess H2(g) 8.00 g of LiH(s) is produced the percent yield is closest to

24.9

An 8.00 sample of copper ore was dissolved in acid solution and then reacted with NO3- from a KNO3 salt solution 3Cu+ 8 NO3- +8H+ → 3 Cu2+ +2NO +4 H2O +6 NO3- it required 71.5 ml of a 0.155 M KNO3 solution to fully react the copper in the ore sample what was the percent copper in the ore

3.30

10 HI+ 2KMnO4+ 3H2SO4 → 5I2 +2MnSO4 + K2SO4 + 8 H2O according to the balanced equation above how many moles of HI would be necessary to produce 2.5 mol of I2 starting with 4.0 mol KMnO4 and 3.0 mol of H2SO4

5.0

CO2(g) + 2LiOH(s) --> Li2CO3(s) + H2O(l) In a person's spacecraft, an astronaut exhales 88.0 g of CO2(g) per day. To prevent the buildup of CO2(g) in a spacecraft a device containing LiOH(s) is used to remove the CO2(g) as represented by the equation above. What mass of LiOH(s) is needed to react with all of the CO2(g) produced by an astronaut in one day

958

A mixture of H2(g) and O2(g) is placed in a container as represented above. The H2(g) and O2(g) react to form H2O(g). Which of the following best represents the container after the reaction has gone to completion.

B

K(s) + 1/2 Cl2(g --> KCl(s) ∆H° = −437 kJ/molrxn What remains in the reaction vessel after equal masses of K(s) and Cl2(g) have reacted until either one or both of the reactants have been completely consumed? (A) KCl only (B) KCl and K only (C) KCl and Cl2 only (D) KCl, K, and Cl2

C

Which of the following particulate diagrams best shows the formation of water vapor from hydrogen gas and oxygen gas in a rigid container at 125 degrees Celcius

C

Which of the following particle diagram best represents the products when four molecules of H2O2(l) decompose into water and oxygen gas at room temperature

D