Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al. Find the theoretical yield (in grams) of manganese from the reaction of 250 g of this mixture.

2 g of aluminium metal is mixed with 11.5 g of sulphuric acid,H2SO4 to form aluminium sulphate and hydrogen gas. a)Write the balanced chemical equation for the reaction.

Write a balanced chemical equation based on the following description: the reaction of aluminum metal with aqueous sulfuric acid to form aqueous aluminum sulfate and hydrogen gas

Based on the balanced reaction: 2 Al + 3 Cl2→ 2 AlCl3, what is the maximum number of moles of AlCl3 that could be made by the reaction of (2.11x10^1) mol of Al and (1.990x10^1) mol of Cl2?

You reduce a 0.9355g solid platinum (IV) oxide with 0.0879g hydrogen gas to yield elemental platinum metal and water vapor in 45% yield. What mass of platinum metal was obtained?

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

How many grams of O2(g) are required to react completely with a piece of magnesium metal that measures 0.10 cm × 1.0 cm × 4.0 cm? The density of magnesium metal is 1.738 g/cm3.

When a solid mixture of MgCO3 and CaCO3 is heated strongly, carbon dioxide gas is given off and a solid mixture of MgO and CaO is obtained. If a 24.00-g sample of a mixture of MgCO3 and CaCO3 produced 12.00 g CO2, what is the percentage by mass of MgCO3 in the original mixture?

A 0.8761 g sample of iron ore is dissolved in acid, the iron is oxidized to the +3 state and then precipitated as Fe2O3·xH2O. This precipitate is filtered, washed and ignited to Fe2O3. The Fe2O3 (159.70 g/mol) weighs 0.1926 g. What is the percentage of iron (Fe, 55.85 g/mol) in the sample?

1 mole of PCI3 is isolated from the reaction of solid elemental phosphorus, P(s), with excess chlorine gas. Determine the moles of phosphorus required for this reaction if the yield is 25%.