For the reaction 4Cr (s) + 3O2 (g) → 2Cr2O3 (s) calculate how many grams of the product form when 24.4 gg of O2O2 completely reacts. Assume that there is more than enough of the other reactant. B) For the reaction 2Sr (s) + O2 (g) → 2SrO (s) calculate how many grams of the product form when 24.4 of SrSr completely reacts. Assume that there is more than enough of the other reactant.

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant.C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 0.0500 molO2 to mol CO2 Express your answer using three significant figures.

A sample of 4.00g of methane (CH4) is mixed with 15.0g of chlorine (Cl2). Determine which is the limiting reactant according to the following equation: CH4(g) + 4Cl2(g)> CCl4(e) + 4HCl(g)

For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant.C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 4.6 molO2 Express your answer using two significant figures.

For the following unbalanced chemical equation, suppose that exactly 1.60 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS, (1) + 02 (9) → CO2(g) + SO2 (g) Limiting reactant: Mass of CO2 = For the following unbalanced chemical equation, suppose that exactly 1.45 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2 (9) → CN, H,O(s) + H2O(1) Limiting reactant: Mass of H2O = b)

For the following reaction, 3.02 grams of carbon monoxide are mixed with excess sulfur. The reaction yields 2.68 grams of sulfur dioxide. sulfur (s) + carbon monoxide (g) →sulfur dioxide (g) + carbon (s) What is the theoretical yield of sulfur dioxide ? grams What is the percent yield of sulfur dioxide ?

Al2Cl6 is made by treating scrap metal with chlorine gas according to the following equation: 2 Al (s)   +   3 Cl2 (g)   ⟶⟶   Al2Cl6 (s)  In the reaction of 45.9 g Al with 212.5 g Cl2, determine the limiting reactant and theoretical yield of the product. The limiting reactant is? The theoretical yield of Al2Cl6 is?.  Round the answer to 1 decimal place. If the reaction produces 139.4 g Al2Cl6, calculate the percent yield of the reaction. ? %.     Round the answer to 1 decimal place.

A) For the reaction Ca(s)+Cl CL2(g)→CaCl2(s) calculate how many grams of the product form when 14.4 g of Ca completely reacts. Assume that there is more than enough of the other reactant. B) For the reaction 2K(s)+Br2(l)→2KBr(s) calculate how many grams of the product form when 14.4 g of Br2 completely reacts. Assume that there is more than enough of the other reactant. C) For the reaction 4Cr(s)+3O2(g)→2Cr2O3(s) calculate how many grams of the product form when 14.4 g of O2 completely reacts. Assume that there is more than enough of the other reactant. D) For the reaction 2Sr(s)+O2(g)→2SrO(s) calculate how many grams of the product form when 14.4 of Sr completely reacts. Assume that there is more than enough of the other reactant.

For the following reaction,14.2 grams of phosphorus (P4) are allowed to react with 34.2 grams ofchlorine gas .phosphorus (P4) ( s ) +chlorine ( g ) phosphorus trichloride ( l)What is the maximum amount of phosphorus trichloride that can be formed? grams What is theFORMULA for the limiting reagent?   What amount of the excess reagent remains after the reaction is complete? grams

What is the mass in grams of CO2 that can be produced from the combustion of 5.26 moles of butane according to the given equation: 2C4H10(g) + 13 O2(g) -> 8CO2(g) + 10H2O(g)