Ans b) 0.136 g
Number of mol of AgNO3 = mass / molar mass
= 0.200 / 169.9 = 0.0012 mol
mol NaOH = 0.200 / 39.997 = 0.005 mol
Number of mol of AgNO3 is less , so it is the limiting reagent here
Number of mol of Ag2O formed = 0.0012 /2 = 0.00059
Mass of Ag2O = mol x molar mass
= 0.00059 x 231.7
= 0.136 grams
When solutions of AgNO3 and NaOH react, the balanced molecular equation is 2AgNO3(aq) + 2NaOH(aq) Ag2O(s) + 2NaNO3(aq) + H2O(l) How much Ag2O is produced when 0.200 g of AgNO3 and 0.200 g of NaOH react
3. When solutions of AgNO3 and NAOH react, the balanced molecular equation is: 2 AgNO3(aq) +2 NaOH(aq)Ag,O(s) + 2 NaNOs(aq) + H20() How much Ag20 is produced when 0.300 g of NaOH reacts with excess silver nitrate? a. 0.869 g b. 1.43 g c. 1.74 g d. 2.30 g
When solutions of H2SO 4 and NaOH react, the balanced molecular equation is: H2SO 4(aq) + 2NaOH(aq) -->Na2SO4(aq) + 2H2O(l) How much Na2SO4 is obtained when 4.00 g of H2SO4 reacts with 2.00 g of NaOH?
2. When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) + AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO, reacts with excess NaCl? a. 1.55 g b. 2.62 c. 4.17 g d.6.20 g
2. When solutions of AgNO3 and NaCl react, the balanced molecular equation is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) How much AgCl is produced when 3.10 g of AgNO3 reacts with excess NaCl? a. 1.55 g b. 2.62 c. 4.17 g d. 6.20 g 1. Given the reaction 2 HgO(s) → 2 Hg(1) + O2(g). What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO? a. 43.8 g b. 78.5 g c. 87.5...
pts) Consider the following balanced equation: Na2SO4 (aq) + 2AgNO3 (aq) → Ag2SO4 (9) + 2NaNO3(aq) a. How many grams of Ag2SO4 result from the reaction of 6.764 g of Na SO, with 15.00 g of AgNO3? b. If the reaction has a 57.3% percent yield, how much Ag2SO4 was actually made? pts) How many grams of O, reacted if 306 kcal are released in the following reaction? CH(g) + 2O2(g) - CO2(g) + 2H2O(l) + 213 kcal
2AgNO3(s)+CoSO4(aq)—Co(NO3)2(aq)+Ag2SO4(s) determine the mass ,in g, of Ag2SO4 produced when 7.47g of AgNO3 react with 50mL of 0.56M CoSO4
Na2SO4(aq) + 2AgNO3(aq) → Ag2SO4(s) + 2NaNO3(aq)Using the balanced equation above, determine the amount of excess reactant remaining when 99.7 g of Na2SO4 reacts with 75.0 g of AgNO3.
5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water is written as HOH(), then the equation is Na(s) + HOH(l) ? NaOH(aq) + H2(g) Write the following reactions: Oxidation reaction: Reduction reaction: Balanced net ionic reaction: Reducing agent: Oxidizing agent:
Write the balanced molecular equation that occurs when aqueous solutions of Y(NO3)3 and K2S react. For full credit, include states (s, l, g, or aq) of all reactants and products, use subscripts for numbers, and use as an arrow
NaOH(aq) + KHP(aq) —> NaKP(aq) + H2O(l) a.) Describe the meaning of the molecular equation between the NaOH and KHP on the microscopic and macroscopic scales, and by mass. b.) Consider the properties of NaOH. Identify reasons why it needs to be standardized before being used in a measurement. c.) Consider the properties of KHP. Identify any properties that make KHP a good choice for the standardizing of a basic solution. d.) This experiment requires an acid-base indicator. Describe how an...