For the following reaction, 3.48 grams of iron are mixed with excess oxygen gas . The reaction yields 3.72 grams of iron(II) oxide. iron ( s) + oxygen ( g ) → iron(II) oxide ( s ) What is the theoretical yield of iron(II) oxide ? What is the percent yield for this reaction ? grams %

The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?

Hexane is a colourless liquid with a characteristic smell that reacts with chlorine gas in the presence of a catalyst. Chlorohexane is a liquid compound that is formed through the substitution of one hydrogen in the hexane molecule with chlorine. Write the chemical equation for this reaction and explain if it requires balancing. Hydrogen chloride gas is also a product of this chemical reaction. Note: ignore the presence of the catalyst.

of 15 An aqueous solution containing 9.88 g of lead(II) nitrate is added to an aqueous solution containing 5.48 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation: What is the limiting reactant? O lead(II) nitrate O potassium chloride The reaction goes to completion, but in the process of washing and drying the precipitate, some was lost. The percent yield for the reaction is 84.8%. How many grams of precipitate are recovered? F precipitate recovered: R V G Search or type URL % 5 T G B MacBook Pro 6 Y H & 7 N U J 8 00 M 1 ( 9 K O V H I ) O L P ^. { لا لا / 1 = ? 11 1 mi

What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?

For the following reaction, 23.0 grams of iron are allowed to react with 5.18 grams of oxygen gas. iron(s) + oxygen (g) → iron(II) oxide(s) What is the maximum mass of iron(II) oxide that can be formed? Mass= g What is the FORMULA for the limiting reactant? What mass of the excess reagent remains after the reaction is complete? Mass= g

Balance the following chemical equation (using the number "1" if the blank normally is left unfilled). Na (s) + NaF (s) F₂ (g) ---->

For the following reaction, 0.557 moles of potassium hydroxide are mixed with 0.224 moles of phosphoric acid. potassium hydroxide(aq)+phosphoric acid(aq)= potassium phosphate(aq)+water(l)   What is the formula for the limiting reagent? What is the maximum amount of potassium phosphate that can be produced?

For the following reaction, 17.5 grams of iron are allowed to react with 37.0 grams of chlorine gas. iron(s) + chlorine(g) → iron(III) chloride(s) What is the maximum mass of iron(III) chloride that can be formed? Mass = 9 What is the FORMULA for the limiting reactant? What mass of the excess reagent remains after the reaction is complete? Mass= g

Your crucible has a mass of 30.252 g when empty, and does not change upon heating. You add some solid iron and then weigh the crucible and iron to be 32.925 g together. You then burn the iron in the presence of oxygen following the procedure in the handout. Assume that there are no contaminates and all of the iron is converted to iron oxide. The final mass of the crucible and iron oxide is 33.976 g, which does not change upon heating. The unrounded empirical formula obtained from these measurements would be FeOX, where X is a decimal type number (not necessarily a whole number). Give the value of X in the blank below in decimal format with the correct number of significant figures.