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How Many Moles of H3Po4 are Produced When 71.0 G

When thinking about acids and bases, one of the first things that comes to mind is the concept of moles. Moles are a unit of measurement that allows chemists to more accurately work with very small numbers of particles. In terms of acid-base reactions, the mole ratio is especially important.

This is because it tells us how many moles of each reactant are needed in order for the reaction to occur. For example, in the neutralization reaction between hydrochloric acid and sodium hydroxide, the mole ratio is 1:1. This means that for every mole of HCl that reacts, one mole of NaOH is also required.

How many grams of Ca are required to react with 12.0 g of oxygen to form CaO?

When 71.0 g of H3PO4 reacts with an excess of NaOH, how many moles of H3PO4 are produced? In order to answer this question, we must first know the chemical equation for the reaction between H3PO4 and NaOH. This equation is as follows:

H3PO4 + 3NaOH → 3H2O + Na3PO4 From this equation, we can see that for every mole of H3PO4 that reacts, three moles of NaOH are required. This means that if we have 71.0 g of H3PO4, we need 213.0 g (71.0 x 3) of NaOH in order to completely react all the H3PO4.

Now that we know the amount of reactants needed, we can calculate the number of moles present using their respective molar masses: 213.0 g NaOH × (1 mol/40.00 g) = 5.325 mol NaOH  7 1 0 . 0 G o f N a O h a r e p r o d u c e d .

 2 1 3 . 0 G / m o l i s t h e m o l a r m a s s o f N a O H .

How Many Grams of H3Po4 are Produced When 10.0 Moles

When 10.0 moles of H3PO4 are produced, the number of grams produced will be 176.6. This is because the molecular weight of H3PO4 is 98.0 g/mol. Therefore, 10.0 moles x 98.0 g/mol = 980 grams of H3PO4 that are produced when 10 moles are made.

How Many Liters of Hydrogen Gas are Needed to React With Cs2 to Produce 2.50 L of Ch4 at Stp?

When looking at how many liters of hydrogen gas are needed to react with cesium to produce methane, it\’s important to consider the standard temperature and pressure (STP). At STP, 2.50 liters of methane can be produced by reacting 4.16 grams of cesium with 8.33 liters of hydrogen gas. To find out how many moles of each element are necessary for the reaction, we can use their molar masses: Cesium – 132.905 g/mol Hydrogen – 2.016 g/mol Methane – 16.043 g/mol By using the mole ratios from the balanced equation for this reaction – CH4 + H2 -> CsH6 – we can determine that for every 1 mol of methane produced, 0.5 mol of hydrogen is required.

How Many Liters of Nh3, at Stp, Will React

If you are looking to find out how many liters of NH3 will react at STP, then you have come to the right place. In this blog post, we will provide you with all of the information that you need in order to make this determination. To begin, it is important to understand what NH3 is and what its properties are.

NH3 is a colorless gas that has a very distinctive odor. It is highly soluble in water and is often used as a household cleaning agent. When NH3 reacts with another substance, it forms a compound known as an ammonium salt.

Now that we know what NH3 is, let\’s take a look at how many liters of it will react at STP. In order to do this, we need to know two things: the molar mass of NH3 and the molar volume of NH3 at STP. The molar mass ofNH 3 ia 17 grams/mol while the molar volume ofNH 3 ia 22.4 liters/mol .

This means that one liter of NH 3 will react with 0.77 mol s-1of other substances under standard conditions (such as temperature and pressure). Now that we know these values, we can easily calculate how many liters of NH 3 would be required to completely react with another substance. For example, if we want to know how many liters ofNH 3 would be needed to completelyreact with 1 liter of water, we would use the following equation:

1 liter H2O x (1 mol H2O / 18 grams H2O) x (17 grams NH3 / 1 molecure) = 0.95 litersNH 3 neededto complete reaction This tells us that approximately 0.95 liters of ammonia would be required in order for it toproperlyreactwith 1 literof water – which isn\’t too bad! However, ifwe wantedto know howmanylitersofammoniarequiredforit toproperlyreactwith 10litersofwater , weneedonly multiplyouranswerby10 :

0 . 95 l i t e r s N H _ { 3 } n e e d e d t o c o m p l e t e r e a c t i o n \\times 10= 9 .

How Many Moles of H3Po4 Would Produce 12 Moles of Water in This Reaction

In this reaction, 3 moles of H3PO4 would produce 12 moles of water. The reason for this is that the molecular weight of H3PO4 is 98 grams/mol, and the molecular weight of water is 18 grams/mol. Thus, 3 moles of H3PO4 would weigh 294 grams, and 12 moles of water would weigh 216 grams.

How Many Moles of Aluminum are Needed to React Completely With 1.2 Mol of Feo

In order to answer this question, we first need to understand what a mole is. A mole is a unit of measurement that equals Avogadro\’s number of particles, which is 6.02 x 10^23. This means that one mole of any substance contains 6.02 x 10^23 atoms or molecules of that substance.

With that said, let\’s calculate how many moles of aluminum are needed to react completely with 1.2 mol of Feo. According to the equation for this reaction, we can see that 2 mol of aluminum are needed for every 3 mol of Feo. Therefore, we need 1.2mol * (2/3) = 0.8 mol of aluminum in order to completely react with 1.2mol of Feo .

How Many Moles of H3Po4 are Produced When 20.0 G of Hcl are Produced by the Reaction?

When 20.0 g of HCL are produced by the reaction, 8.0 moles of H3PO4 are also produced.

How Many Moles of O are Present in 4.9 G of H3Po4?

There are three moles of oxygen atoms for every mole of phosphoric acid, so there would be 9 moles of oxygen atoms in 4.9 g of H3PO4.

How Many Grams of H3Po4 are Produced When 10.0 Moles of Water React With an Excess of P4O10?

In a chemical reaction, the limiting reagent is the substance that is completely used up when the reaction reaches equilibrium. The other reactant is in excess and its quantity does not change during the reaction. In a displacement reaction, the more reactive element displaces the less reactive element from a compound.

When 10 moles of water react with an excess of P4O10, 8 moles of H3PO4 are produced.

What Mass of Phosphoric Acid H3Po4 98.00 G Mol is Produced from the Reaction of 10.00 G of P4O10 283.89 G Mol With 12.00 G Water?

In order to answer this question, we must first understand the reaction that is taking place. The equation for this reaction is as follows: P4O10 + 6H2O -> 4H3PO4

This equation tells us that one mole of P4O10 will react with six moles of water to form four moles of phosphoric acid. Therefore, we can say that the ratio of reactants is 1:6:4. With this information, we can now calculate the amount of each reactant needed to produce a given amount of phosphoric acid.

In this case, we know that we are starting with 10.00 g of P4O10 and 12.00 g of water. We can convert these masses into moles using their respective molecular weights (283.89 g/mol for P4O10 and 18.02 g/mol for H2O). This gives us 0.035 moles of P4O10 and 0.667 moles of H2O.

Since the ratio of reactants is 1:6:4, we know that we need six times as much water as phosphorus pentoxide in order to complete the reaction.


When 71.0 grams of phosphorus pentoxide are heated with an excess of water, 45.3 grams of phosphoric acid are produced. This is equivalent to 0.500 moles of H3PO4.