The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below:                               P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 110.03 grams P4S3with excess O2? a. 220.06 g b. 164.060 g c. 66.18 g d. 392.18 g e. 96.000 g

21. Tungsten reacts with Cl2 to form WCl6 according to the following balanced equation: W  + 3 Cl2  ==> WCl6 Determine the mass of WCl6 that forms when 231.80 g of W completely react.   Molar Mass, g/mol W 183.91 Cl2 70.91 WCl6  396.56

Synthesis of disulfur diclhoride S8 + 4Cl2 —> 4 S2 Cl2 0.7797 mol S8 and 1.410 mol Cl2 are combined to make S2Cl2 1.What is the limiting reactant? 2.How much excess reactant will be left 3. How many moles of product can be made

Calculate how many grams of O2(g) can be produced from heating 33.7 g KCIO,(s).

A compound is composed of the elements, carbon, hydrogen, and chlorine only. Combustion of the compound produces CO2, H2O, and HClC?H?Cl? + O2 ➝ CO2 + H2O + HCl Combustion of a 10.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 19.549 H2O 5.502 HCl 4.049         Determine the empirical formula for the compound

6. The gaseous hydrocarbon acetylene (C2H2) used in welders' torches, burns according to the following equation: 2C2H2(g) + 502(g)→ 4CO2(g) + 2H2O(g) a. What is the theoretical yield, in grams, of CO2, if 22.0 g of C2H2 completely reacts? b. If the actual yield in part a is 64.0 g of CO2, what is the percent yield of CO2 for the reaction?

3. How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.642 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (9) + 2H₂O(1) mol CH4 mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.622 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.618 mol of the first reactant were to react completely. C3H8 (g) + 5O2(g) → 4H₂O(1) + 3CO₂ (9) mol H₂O mol CO₂

A sample of 5.0 g of hydrogen gas reacts with 5.0 g of oxygen gas. 2H2 (g) + O2 (g) → 2H2O(l) d. How much excess reactant remains? e.If 4.2 g of water is actually produced, what is the percent yield?

a. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.255 mol of the first reactant. AgNO3(aq) + LiOH(aq) → AgOH(s) + LiNO3(aq) g AgOH g LINO3 b. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.155 mol of the first reactant. Al2(SO4)3(aq) + 3CaCl₂ (aq) → 2AlCl3 (aq) + 3CaSO4 (8) g AICI, g CaSO4 c. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.215 mol of the first reactant. CaCO3 (8) + 2HCl(aq) → CaCl2 (aq) + CO2(g) + H₂O(l) g CaCl2 g CO2 g H₂O Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next > Save and Exit